Investigation of CH₄ Hydrate Formation Under the Synergistic Effects of Graphite Nanofluids and Cyclopentane and Its Storage Stability at Subzero Temperatures

Abstract

The solidified natural gas (SNG) technology presents a prospective strategy for CH₄ storage and transportation. Low gas storage capacity and slow formation rate remain the key challenges for its field applications. This study suggested a compound system of cyclopentane (CP) + graphite nanoparticle (GNP) nanofluid to enhance the formation kinetics of CH₄ hydrate. Results indicated that both gas consumption and hydrate formation rate were higher at a higher CP concentration, peaking at 14 wt%, where t₉₀ (the time to reach 90% of the final gas uptake) was 65.7 min, and the gas uptake reached 0.1346 mol/mol. However, an excessive CP (21 wt%) negatively affected CH₄ hydrate generation kinetics due to the excessive cage occupancy of CP in 5¹²6⁴ cavities. A lower temperature was determined to be more favorable for CH₄ hydrate formation within nanofluids, which was visually demonstrated by the denser hydrate crystals formed at 275.15 K. Moreover, storage stability analysis revealed that CH₄ hydrate formed in CP + GNP nanofluids can be preserved at atmospheric pressure and 268.15 K without significant decomposition. This work provides a superior scheme for hydrate-based CH₄ storage, offering great contributions to SNG technology advancement.

1. Introduction

Gas hydrates are ice-like crystalline compounds formed by water and gas molecules (such as CH₄, CO₂, etc.) under high-pressure and low-temperature conditions [1,2]. Gas hydrates are typically categorized into sI, sII, and sH, three types [3,4,5,6,7]. Hydrate formation is widely recognized as an effective method for natural gas storage and transportation, namely Solidified Natural Gas (SNG) technology [8,9,10]. Compared to traditional natural gas storage technologies like CNG and LNG, SNG shares the advantages of high capacity [11], mild conditions [12,13], and greater convenience in storage and transportation. However, harsh conditions associated with hydrate formation and its slow rate are the bottlenecks that must be overcome prior to field application of the SNG technology [14,15,16].

Using thermodynamic promoters is an effective means of modifying the hydrate phase equilibrium, facilitating hydrate crystallization under more moderate conditions, and hence lessening the expense associated with hydrate formation [17,18,19,20]. Tetrahydrofuran (THF) has been widely employed to moderate CH₄ hydrate phase equilibrium and facilitate CH₄ hydrate formation [21,22]. The equilibrium pressure of methane hydrate was found to drop from 6.9 MPa to around 0.5 MPa at 283.15 K with 5.56 mol% THF [23], which accelerates CH₄ hydrate formation. Another environmentally friendly thermodynamic promoter, dioxane (DIOX), has been utilized to moderate formation conditions [24]. With 5.56 mol% DIOX, the equilibrium pressure of CH₄ hydrate at 283.15 K decreases to 1.0 MPa, which is less pronounced than that with THF [25]. Recently, cyclopentane (CP) was found to outperform THF in reducing CH₄ hydrate formation pressure [26]. It was reported that the equilibrium curve for methane hydrate in solutions containing CP exhibits a significant shift toward the thermodynamically favorable area, in contrast to that without CP. The equilibrium conditions for methane hydrate within a 5.6 mol% CP solution were determined as 0.62 MPa and 287.25 K [27]. As presented, CP shifts the phase equilibrium more significantly than DIOX and comparably to THF. Furthermore, the low water solubility and volatility of CP enable its easy separation and reuse. Therefore, CP is less toxic and more readily recoverable than THF and DIOX, aligning with the green chemistry principles. [28].

Nanofluids have been successfully utilized to enhance CH₄ hydrate formation kinetics, accelerating the process and improving gas consumption efficiency [29,30,31,32]. The addition of nanoparticles enhances heat transfer during hydrate formation, while the dispersed nanoparticles provide numerous nucleation sites, thereby accelerating hydrate crystallization and improving formation kinetics [33,34,35]. Metal nanoparticles, including Fe₃O₄ [33], ZnO [34], and CuO [36], are commonly used to optimize the CH₄ formation kinetics. It was found that SDS@Fe₃O₄ induced a faster hydrate nucleation and higher gas consumption than SDS alone [33]. In addition, the gas consumption of CH₄ hydrate formation within a 500 ppm SDS + 0.3 wt% CuO nanofluid was 12.2% higher than that in a 500 ppm SDS solution [36]. However, the high cost and environmental pollution of metal nanoparticles limit their widespread application [37]. In contrast, graphite nanoparticles are considered biocompatible, cost-effective, and easily produced, with excellent thermal conductivity, which helps promote hydrate growth [38,39,40,41]. Research revealed that, in comparison with pure water, the use of GNP reduced the induction time by 80.8% and increased gas uptake by 12.8% [38]. One study indicated that adding GNP to THF solution increased gas storage by 36% and curtailed the t_ind compared to the THF solution alone. [40]. Moreover, comparison between GNP and metal nanoparticles has highlighted that, under identical temperature and pressure conditions, gas consumption achieved in the GNP nanofluid system was 8~30% higher than that in ZnO and CuO nanofluid systems [42].

As observed, the validity of CP in controlling hydrate formation conditions and GNP in enhancing hydrate formation kinetics has been established independently. However, the synergistic improvement of CP + GNP combination on hydrate formation has not been reported yet, and CH₄ hydrate growth kinetics in CP + GNP nanofluids remain unexplored. This study examined the synergistic impact of GNP and CP on CH₄ hydrate generation. Gas consumption and hydrate formation rates in GNP nanofluids were measured. Additionally, hydrate formation kinetics in CP + GNP nanofluids were investigated at various temperatures. Finally, the stability of CH₄ hydrate storage in CP + GNP nanofluids under atmospheric pressure was assessed. This study is conducive to elucidating the synergistic effect of GNP and CP on CH₄ hydrate formation and will offer deeper insights into the SNG technology advancement.

2. Experimental Section

2.1. Materials

CH₄ gas (99.99 mol%) was offered by Chongqing Jiarun Gas Co., Ltd., Chongqing, China. Graphite nanoparticles (GNP, 99.95% purity) with an average size of 50 nm were purchased from Xuzhou New Material Technology Co., Ltd., Xuzhou, China [40], and the SEM images can be seen in our previous study [40]. It was shown that graphite nanoparticles exhibit uniform distribution and a plate-like structure, with one dimension measured less than 500 nanometers. Sodium dodecyl sulfate (SDS, 99% purity) and cyclopentane (CP, 96% purity) were supplied by Chengdu Chemical Co., Ltd., Chengdu, China. According to the zeta potential measurement and stability evaluation, GNP nanofluid exhibits good colloidal stability over 24 h [43,44], so they can exist stably within the experimental period. Distilled water (with 18.2 MΩ·cm resistivity) was applied for all experiments.

2.2. Apparatus

The formation and dissociation of CH₄ hydrate were investigated using a microscopic experimental setup. This apparatus has been documented in the previous literature [45,46]. Briefly, a 100 cm³ transparent sapphire reactor is the core part of the setup, with the maximum working pressure of 10 MPa [47]. A stereomicroscope and a CCD camera were mounted in front of the water bath to photograph images of hydrate crystals [47].

2.3. Procedures

2.3.1. Preparation of GNP + CP Nanofluids

GNP + CP nanofluid was produced using a two-step method. The specific steps are as follows: (1) Prepare an SDS solution with the SDS concentration fixed at 500 ppm, which is an optimal concentration to form a stable nanofluid. This has been verified in our previous study [9]; (2) Measure the required amount of GNP and add it to the SDS solution; (3) Stir the mixed solution with a magnetic stirrer for 15 min; (4) Disperse the solution ultrasonically for 20 min to create the graphite nanofluid; (5) Add a specified amount of CP to the graphite nanofluid to form the combined GNP + CP nanofluid.

2.3.2. Kinetic Experiments for CH₄ Hydrate Formation

Hydrate formation experiments were conducted as follows. The reactor was first rinsed with distilled water, followed by the injection of 100 mL of GNP+CP solution. Subsequently, three purges with CH₄ were performed to eliminate air. Pressurizing the reactor to 6 MPa using CH₄ as it was cooled to the set value. Launched the agitation and adjusted its speed to 300 rpm. Temperature and pressure data were recorded by data acquisition system every 10 s. Each experimental group was repeated three times under identical conditions to verify reproducibility. The first run was designated as the “fresh,” while the subsequent two runs were designated as “memory.”

The amount of CH₄ consumed during hydrate formation is calculated using Equation (1).

$$\mathrm{NGC}={\displaystyle \frac{\Delta n_{\mathrm{H}}}{n_{\mathrm{w}}}}={\displaystyle \frac{n_{\mathrm{g},0}-n_{\mathrm{g},t}}{n_{\mathrm{w}}}}={\displaystyle \frac{{\left(\frac{PV}{ZRT}\right)}_0-{\left(\frac{PV}{ZRT}\right)}_t}{n_{\mathrm{w}}}}(\mathrm{mol}\mathrm{gas}/\mathrm{mol}\mathrm{water})$$

(1)

where Δn_H represents the molar amount of gas molecules captured in hydrate at the end of the experiment, n_w denotes the water amount used in the experiment, n_g,0 and n_g,t denote the methane gas amount in the reactor at time 0 and time t, respectively, P is the pressure, T and V are the temperature and volume of gas phase, R is ideal gas constant, and Z is the compressibility factor calculated utilizing Pitzer correlation in Equation (2).

$$Z=1+B^0{\displaystyle \frac{P_r}{T_r}}+\omega B^1{\displaystyle \frac{P_r}{T_r}}$$

(2)

Abbott’s equations are used for the calculation of B⁰ and B¹ [48].

According to the study reported in the literature [49,50], under the experimental conditions (6 MPa, 275–279 K), the uncertainty in Z is estimated to be less than 2%, which represents a negligible error in the gas uptake calculation.

Gas storage capacity is the phase volume ratio of the gas-hydrate, as calculated by Equation (3).

$$V_{\mathrm{GH}}={\displaystyle \frac{V_{\mathrm{gas}}}{V_{\mathrm{H}}}}={\displaystyle \frac{(22.4\times 1000)}{[(M_{\mathrm{W}}/{\rho }_{\mathrm{W}}+\Delta V)\times N]}}$$

(3)

where V_GH is storage capacity, V_gas is the gas volume stored in the hydrate under standard conditions, V_H is the hydrate volume, M_W and ρ_W are the molar mass and density of water. ΔV is the difference between the molar volumes of the hydrate and the liquid phase, and was set to 4.6 cm³/mol [51]. N is hydrate number [42].

2.3.3. Morphology Experiments of CH₄ Hydrate Formation

The solution used in the experiments was 0.5 wt% GNP + 14 wt% CP. After cleaning the reactor three times with pure water, 60 mL of the solution was introduced. The reactor was then purged 3 times by CH₄ to remove residual air. After cooling the solution to the target temperature, the reactor was pressurized to 6 MPa using CH₄. The magnetic stirrer began to stir the contents of the reactor at 300 rpm. The camera captured and recorded the morphology of the hydrate crystals every 5 s.

2.3.4. Experiments on CH₄ Hydrate Storage

CH₄ hydrate formation at 277.15 K, 6.0 MPa was described in Section 2.3.2. After hydrate generation, chill the reactor to a designated subzero temperature, which refers to that below 273.15 K, for 12 h. Subsequently, rapid depressurization to 0.1 MPa was performed. Finally, CH₄ hydrate was stored at 0.1 MPa and the desired temperature for 48 h.

The gas recovery (R%) from hydrate dissociation is calculated by Equation (4).

$$R\%={\displaystyle \frac{n_{\mathrm{dissociation}}}{n_{\mathrm{formation}}}}\times 100\%$$

(4)

where n_formation is the amount of the gas consumption during hydrate generation, and n_dissociation is the gas amount that is recovered after dissociation.

3. Results and Discussion

3.1. Effects of CP on CH₄ Hydrate Formation in Graphite Nanofluids

The t_ind, t₉₀, gas consumption, and gas storage capacity gained from the experiments are listed in

Table 1. Experiment conditions and results in different systems. All experiments were conducted at 277.15 K and 6 MPa.

Exp. No.	Exp. State	CP Concentration (wt%)	tind (min)	t90 (min)	NGC (mol of Gas/mol of Water)	Gas Storage Capacity (V/V)
1#	fresh a	0	1.3	77.2	0.1131	112.2
2#	memory b		1.7	78.0	0.1130	112.0
3#	memory		1.0	80.2	0.1131	112.2
4#	fresh	7	1.0	76.5	0.1227	121.6
5#	memory		1.3	71.5	0.1210	119.9
6#	memory		1.0	72.2	0.1199	118.5
7#	fresh	14	0.8	63.0	0.1349	133.9
8#	memory		1.2	62.0	0.1326	131.6
9#	memory		1.0	72.2	0.1362	135.0
10#	fresh	21	0.5	48.0	0.1289	127.9
11#	memory		0.7	84.2	0.1298	128.6
12#	memory		0.8	65.2	0.1289	127.9

^a The solution was used for hydrate formation for the first time. ^b The solution had experienced hydrate formation previously.

. Figure 1 displays the effects of CP concentration on CH₄ consumption in GNP + CP nanofluids. As seen in Figure 1a, during the initial 20 min, an increased CP concentration led to a faster reaction rate and greater gas consumption. This can be attributed to the fact that elevated CP concentrations lead to the formation of more CP hydrates within the GNP nanofluid, thereby facilitating the entry of CH₄ into the pre-formed hydrate cage structures. At the same time, the increased amount of CP can aid in transferring more CH₄ molecules into solution for subsequent incorporation with water. As the experiment progressed, gas consumption in the 0.5 wt% GNP + 14 wt% CP system surpassed the 0.5 wt% GNP + 21 wt% CP system after approximately 30 min, showing the enhanced formation kinetics. Finally, as depicted in Figure 1b, gas consumption in 0.5 wt% GNP + 14 wt% CP system was 4.2% higher than that of the 0.5 wt% GNP + 21 wt% CP system. This mainly resulted from the increased mass transfer impedance during hydrate generation in the 0.5 wt% GNP + 21 wt% CP system, resulting in a smaller cage occupancy of CH₄ compared with that of the 0.5 wt% GNP + 14 wt% CP system.

Figure 2 shows temperature variations over CH₄ hydrate generation at varied CP concentrations. As presented in Figure 2a, in the 0.5 wt% GNP nanofluid without CP, a temperature peak appeared at 20.8 min and it reached the maximum value of 278.63 K, indicated by black arrows. This suggests the substantial and continuous hydrate generation during this period [52]. When adding a certain amount of CP into the GNP nanofluid, as exhibited in Figure 2b–d, the temperature peak reached 278.79 K, 278.86 K, and 279.04 K, corresponding to 7 wt%, 14 wt%, and 21 wt% CP, respectively, higher than that in the 0.5 wt% GNP nanofluid without CP. This indicates greater hydrate formation with increased CP concentration. It is also found that a higher CP concentration resulted in a shorter time to reach the maximum temperature of the exothermic peak. For example, the time obtained at 0, 7 wt%, 14 wt%, and 21 wt% CP was 20.8 min, 13.0 min, 10.2 min, and 8.5 min, respectively, indicating that higher CP concentrations can facilitate faster hydrate formation during the initial phase.

Figure 3 compares t₉₀ at varied CP concentrations. Obviously, t₉₀ decreased as the CP concentration increased from 0 to 21 wt%. t₉₀ obtained at 7 wt% CP was 73.4 min, and it decreased to 65.7 min as the CP concentration increased to 14 wt%, indicating a reduction of 10.5%, also showing a decrease of 16.3% compared to that obtained in 0.5 wt% GNP nanofluid without CP. This is because a greater CP hydrate formed in a denser CP solution, providing a larger number of hydrate cages to trap CH₄ molecules. Thus, the process of hydrate formation was shortened. However, t₉₀ obtained at 21 wt% CP was 65.8 min, nearly identical to that observed at 14 wt% CP. This means that the promoting effect cannot be enhanced while the CP concentration exceeds 14 wt%.

Figure 4 compares the gas storage capacity obtained within GNP nanofluids containing varied CP concentration. As seen, at 7 wt% CP, gas storage capacity reached 120 V/V, which was 7% larger than that obtained in the absence of CP (112.1 V/V), indicating that gas storage capacity elevated in the presence of CP. Interestingly, the gas storage capacity at 14 wt% CP (133.5 V/V) was greater than that acquired at both 7 wt% and 21 wt% CP, demonstrating that 14 wt% was an optimum concentration to increase the gas storage capacity among all the tested CP concentrations. This phenomenon can be attributed to two mechanistic constraints. Firstly, increased CP concentration lowers the aqueous phase volume, reducing the quantity of water available for hydrate formation with CH₄. Secondly, CP acts as a competing guest molecule for the large hydrate cages. At higher concentrations, CP occupancy of these cages increases, which in turn suppresses CH₄ inclusion [53]. Although increasing the CP concentration enhanced hydrate nucleation and growth, the highest gas storage capacity was achieved at the medium concentration of CP (14 wt%). Based on this result, it is believed that when the GNP + CP system is applied to enhance CH₄ hydrate formation, the CP concentration should be maintained at 14 wt%, which is conducive to obtaining a higher CH₄ gas storage capacity.

3.2. Impacts of Temperature on CH₄ Hydrate Formation in GNP + CP Nanofluids

0.5 wt% GNP + 14 wt% CP system demonstrated superior performance in boosting CH₄ hydrate generation. However, the impact of temperature on CH₄ hydrate generation remains unclear.

Table 2. Experiment conditions and results in the 0.5 wt% GNP nanofluid added with 14 wt% CP at different temperatures.

Exp. No.	Exp. State	Temperature (K)	tind (min)	t90 (min)	NGC (mol of Gas/mol of Water)	Gas Storage Capacity (V/V)
1#	fresh	275.15	0.7	27.2	0.1355	134.3
2#	memory		0.4	28.2	0.1378	136.5
3#	memory		0.3	27.8	0.1365	135.2
4#	fresh	277.15	0.8	63.0	0.1349	133.9
5#	memory		1.2	62.0	0.1326	131.6
6#	memory		1.0	72.2	0.1362	135.0
7#	fresh	279.15	1.5	108.3	0.0909	90.0
8#	memory		1.2	87.8	0.0901	89.3
9#	memory		1.2	67.3	0.0914	90.6

presents a comparison of hydrate formation at different temperatures (275.15 K, 277.15 K, and 279.15 K) in this mixed solution.

Figure 5 illustrates the temperature profiles for CH₄ hydrate generation in the 0.5 wt% GNP + 14 wt% CP mixed system. The gray curve represents the temperature profile for CH₄ hydrate formation at 275.15 K, where a sharp peak is observed, suggesting the rapid hydrate generation event. This is primarily due to the increased driving force at a lower temperature, which accelerated hydrate nucleation and, as a result, led to a faster temperature rise. Meanwhile, the rapid hydrate growth allowed the reaction to complete within a short time, followed by a fast recovery of the temperature to the designed value. As the temperature rose to 277.15 K, the temperature peak (red line) was shorter compared to that at 275.15 K, along with an extended recovery period to the original temperature. This indicates that hydrate crystallization at 277.15 K proceeded more slowly, and the hydration reaction required more time to complete. At 279.15 K, the temperature curve (blue line) exhibited several minor temperature peaks, marked by black arrows, indicating continuous nucleation and multiple crystallization events of CH₄ hydrate. On the other hand, hydrate formation at 279.15 K appeared to occur intermittently over approximately 100 min, indicating the slowest hydrate formation among the three temperatures. This is probably caused by the reduced driving force compared to 275.15 K and 277.15 K.

Figure 6 displays the impacts of temperature on CH₄ consumption in 0.5 wt% GNP + 14 wt% CP solution. As seen, gas consumption at 275.15 K (0.1366 mol/mol) was the highest, surpassing that at 279.15 K (0.0908 mol/mol) by 50.4%. Moreover, the rate of gas consumption at 275.15 K was the fastest, indicating that hydrate formed more rapidly at this temperature compared to 277.15 K and 279.15 K. This is because of the higher degree of subcooling at 275.15 K, strengthening the hydrate generation driving force, and thereby inducing a faster generation rate. It is noteworthy that the final gas uptake at 275.15 K and 277.15 K showed a negligible difference, suggesting that despite the stronger driving force at 275.15 K, the amount of gas hydrate did not increase significantly. In contrast, gas consumption at 279.15 K was reduced significantly compared to that at 275.15 K and 277.15 K, indicating that hydrate formation at 279.15 K was less pronounced than that at lower temperatures. This agrees well with the temperature profile presented in Figure 5.

Figure 7 illustrates the impact of temperature on t₉₀ for CH₄ hydrate formation. As observed, t₉₀ at 275.15 K was 27.7 min, significantly shorter than that at 279.15 K (87.8 min). This can be attributed to the faster dissolution and dispersion of CH₄ molecules in the solution at lower temperatures, which also provides a greater driving force for hydrate generation [52]. Further, the longest t₉₀ occurred at 279.15 K, accompanied by the lowest observed gas consumption (as shown in Figure 7), indicating that high temperatures were not favorable for hydrate formation within 0.5 wt% graphite nanofluid + 14 wt% CP system. Consequently, lowering the temperature was effective in enhancing hydrate formation kinetics.

Figure 8 shows the impact of temperature on gas storage capacity for methane hydrate formation in a 0.5 wt% GNP + 14 wt% CP system. As the temperature decreased, the gas storage capacity at 277.15 K reached 133.5 V/V, showing a 48.3% increase compared to that at 90.0 V/V at 279.15 K. This suggests that lowering the temperature can increase the gas storage capacity, primarily resulting from the significant increase in driving force (subcooling) of hydrate formation. However, further cooling to 275.15 K resulted in only a marginal 1.3% rise in gas storage capacity compared to that at 277.15 K, implying that the way of lowering temperature has limited effectiveness in gas storage improvement. This means that hydrate formation at 277.15 K reached a threshold of water conversion to hydrate, and it is very hard to overcome the heat and mass transfer barriers by reducing the temperature, although the hydrate generation rate at 275.15 K was greater compared to that at 277.15 K.

Figure 9 shows the morphological behavior during CH₄ hydrate generation in a 0.5 wt% GNP + 14 wt% CP system under varied temperatures. Note that the kinetic behavior of CH₄ hydrate formation can be elucidated by observing the hydrate growth morphology without using any image analysis metrics [27,46]. Although quantitative image analysis was not performed, the visual comparison clearly indicated that hydrate coverage became more extensive and the crystal density was higher at 275.15 K, consistent with the kinetic data, showing a faster growth and higher gas consumption. Figure 9a,f,k show the beginning of the experiments. It is clear to see that hydrate initially formed at gas/liquid interface because of the extensive contact area, as illustrated in Figure 9b,g,l. At 275.15 K, hydrate crystals appeared at 15 s, while they first appeared at 90 s as the temperature increased to 279.15 K. This means the lower the temperature, the shorter the hydrate induction time. Note that hydrate initially grew upward along the reactor wall, and a small amount of hydrate crystals grew downwards at the same time, as shown in Figure 9c,h,m. As the reaction progressed, the hydrate continued to grow both upward and downward. It was found that lower temperatures resulted in faster hydrate growth, as exhibited in Figure 9d,i,n. Finally, at 600 s, the hydrate nearly covered the reactor wall. However, the hydrate formed at 275.15 K was found to be denser, leaving no additional voids in the reactor. In contrast, the hydrate formed at 277.15 K and 279.15 K did not fully cover the reactor wall, as indicated in the yellow circles in Figure 9j,o. This indicates less hydrate generation at these two temperatures compared to that at 275.15 K. The analysis of the morphological behavior of hydrate generation at varied temperatures revealed that lower temperatures significantly enhanced crystallization kinetics and promoted hydrate growth. These morphological observations are consistent with the kinetic experimental results shown in Figure 6.

According to the revealed evolution patterns and kinetic mechanisms of hydrate formation, Figure 10 elucidates the mechanism of CH₄ hydrate generation in the GNP + CP system. Figure 10a illustrates the initial state of the GNP + CP system, where the CP phase, being both buoyant and water-immiscible, floated on top of the aqueous nanofluid. Figure 10b depicts the onset of the reaction, where CH₄ molecules diffuse through the CP phase and come into contact with water, leading to hydrate generation at the CP/nanofluid interface. CP molecules quickly occupied the 5¹²6⁴ cavities of the hydrates (the large cage consists of 12 pentagonal faces and 5 hexagonal faces, which is assembled from numerous water molecules with hydrogen bonds), while some CH₄ molecules were confined within the 5¹² cavities. At this stage, sII hydrates were predominantly formed. Figure 10c illustrates the intermediate and later stages of hydrate formation. The initially formed sII hydrates caused a reduction in the CP phase, making it difficult to fully cover the CP-nanofluid interface. Subsequently, CH₄ molecules were consumed to form sI hydrates with the remaining water until the reaction was complete. As a result, the sI and sII hydrates ultimately coexisted in the reactor.

3.3. Gas Consumption Comparison in Different Systems

Table 3. Gas uptake of CH₄ hydrate formation in varied systems.

System	Temperature (K)	Pressure (MPa)	Gas Consumption (mol/mol)	Average Hydrate Formation Rate (mmol/min·mol)
GNP + CP a (this work)	277.15	6.0	0.1346	2.1
GNP b (this work)	277.15	6.0	0.1131	1.5
CP c [16]	274.15	7.2	0.1084	1.8
THF d [21]	277.2	8.0	0.0651	1.4
CP + THF e [54]	273.2	7.2	0.0182	0.7
DIOX f [23]	280.2	5.25	0.0489	0.9

^a The concentrations of GNP and CP were 0.5 wt% and 14 wt%, respectively. ^b GNP concentration was 0.5 wt%. ^c CP concentration was 18.7 wt%. ^d THF concentration was 19.1 wt%. ^e The concentrations of CP and THF were 10.7 wt% and 2.0 wt%, respectively. ^f The concentration of DIOX was 22.4 wt%.

compares the gas uptake and average rate for CH₄ hydrate generation across different systems. As seen, the largest gas consumption (0.1346 mol/mol) and the fastest hydrate formation (2.1 mmol/min·mol) are obtained from the GNP + CP system among all the systems listed. This indicates that CH₄ hydrate formation is significantly enhanced in the GNP + CP compound system. At 277.15 K and 6 MPa, the GNP + CP system exhibits a 19.0% increase in gas consumption and a 16.7% increase in formation rate compared to the CP solution. Likewise, CH₄ hydrate formation within the THF, CP + THF, and DIOX systems is also inferior to that within the GNP + CP system. Note that a lower gas consumption and formation rate were obtained, although higher driving forces were reserved in the CP, THF, and CP + THF systems. This means a larger amount of energy was consumed in these systems, but the gas consumption was smaller. As presented, GNP is effective in enhancing CH₄ hydrate formation kinetics, and its combination with CP will become a superior strategy for the high-efficiency CH₄ solidified storage and transportation.

3.4. Stability of CH₄ Hydrate Storage at Atmospheric Pressure

To examine the effectiveness of CP + GNP nanofluids for solidified natural gas storage and transportation, the storage stability of CH₄ hydrate formed within the CP + GNP nanofluid under atmospheric pressure was investigated.

Figure 11 compares the CH₄ gas evolution at 271.15 K, 268.15 K, and 265.15 K under 0.1 MPa. As shown, CH₄ hydrate experienced a significant dissociation during the initial 4 h, where gas evolutions across all storage runs were <16%. Thereafter, the gas evolution curve gradually flattened, indicating a small degree of CH₄ hydrate dissociation. After 48 h, the final gas evolution, ranked from highest to lowest, was 271.15 K (31.2%) > 265.15 K (21.7%) > 268.15 K (10.4%), as summarized in

Table 4. Stability of CH₄ hydrate stored at 0.1 MPa and different temperatures.

Storage Temperature (K)	271.15	268.15	265.15
gas consumption for hydrate formation (mol/mol)	0.1354	0.1371	0.1421
reactor pressure after 2 days storage (kPa)	104	484	895
moles of gas evolution after 2 days of hydrate dissociation (mol/mol)	0.0422	0.0143	0.0308
gas evolution after 2 days of storage	31.2%	10.4%	21.7%
reactor pressure after hydrate dissociation (kPa)	2899	2980	3096
gas recovered from hydrate dissociation (mol/mol)	0.1324	0.1361	0.1414
gas recovery from hydrate dissociation	97.8%	99.3%	99.5%

. Note that CH₄ hydrate decomposed slightly during storage, suggesting that CH₄ hydrate formed within the GNP + CP nanofluid can be effectively preserved at atmospheric pressure under the experimental conditions. This can be induced by the self-preservation effect [55], which prevents rapid hydrate decomposition. At temperatures < 273.15 K, water molecules that were not incorporated into the hydrate and produced from hydrate dissociation quickly formed an ice shell on the methane hydrate surface [56]. The ice layer acts as a physical obstacle, isolating the inner hydrate from the external environment. Consequently, thermal exchange between the surroundings and CH₄ hydrate was restricted, so the hydrate dissociation was hampered.

Note that the optimal temperature for CH₄ hydrate storage at 0.1 MPa in the CP + GNP nanofluids was determined to be 268.15 K, as shown in Table 4. This is probably because excessive ice crystals formed at 265.15 K, which compressed and disrupted the CH₄ hydrate lattice, thus weakening the self-preservation effect and triggering hydrate decomposition [57,58]. This observation also complies with the findings obtained in the literature [59], in which CH₄ hydrate decomposed more fiercely at 266 K than at 269 K. On the contrary, at 271.15 K, the increased thermal motion of CH₄ and water molecules weakened the hydrogen bonds, making the hydrate lattice more prone to collapse and thus facilitating the release of CH₄ molecules trapped in the hydrates.

3.5. Perspectives for Scale-Up

This study demonstrates the promising kinetics and stability of the CP + GNP nanofluid system at the laboratory scale. To advance this technology toward practical application, key challenges must be addressed: (1) ensuring uniform nanoparticle dispersion in large-scale or continuous reactors for consistent performance; (2) developing efficient cyclopentane recovery and recycling processes to reduce cost and environmental impact; and (3) evaluating the long-term stability, safety, and lifecycle of graphite nanoparticles in industrial settings. Successfully overcoming these hurdles is essential for scaling the CP + GNP system into a commercially viable SNG storage technology.

4. Conclusions

This study investigates the synergistic impact of graphite nanofluids and cyclopentane on methane hydrate generation. It was found that adding CP into the GNP nanofluid can significantly enhance hydrate generation. At a combination of 0.5 wt% GNP + 14 wt% CP, the highest gas uptake of 0.1346 mol/mol and storage capacity of 133.5 V/V were achieved. However, an overconcentrated CP concentration of 21 wt% is detrimental to CH₄ hydrate formation because of the excessive cage occupation of CP. Decreasing temperature can promote CH₄ hydrate generation in the CP + GNP nanofluid, with a marginal increase in gas storage capacity between 277.15 K and 275.15 K, suggesting a practical operational threshold. Morphological analysis confirmed that hydrate formation was faster and denser at lower temperatures, which is consistent with the kinetic data. Additionally, the CP + GNP system exhibited excellent storage stability under atmospheric pressure, presenting minimal hydrate disruption at 268.15 K over 48 h, leveraging the self-preservation effect. The findings suggest that the CP + GNP nanofluid system holds significant potential for SNG storage, providing a promising strategy for advancing the SNG technology toward practical applications.