液化循环的研究和热力学分析:能量和能量研究研究
Mehdi Mahboobtosi1, D D Ganji1, Mofid Gorji1
1Department of Mechanical Engineering, Babol Noshirvani University of Technology, Babol, Iran.
Heliyon
|September 24, 2024
概括
这项研究分析了三种液化循环,发现循环3提供了优越的冷却前能量效率. 尽管有所改善,但在所有周期的冷冷却过程中,超过50%的运动能量都会丢失.
科学领域:
- 热力学是一种热力学.
- 能源工程 能源工程
- 化学工程是化学工程的重要组成部分.
背景情况:
- 对像气这样的清洁能源需求不断增长,需要高效的液化.
- 化石燃料能源和环境污染推动了对替代燃料的研究.
- 对液化循环的热力学分析对于优化性能至关重要.
研究的目的:
- 对三种不同的液化循环进行热力学研究.
- 评估和比较不同预冷和冷冷却配置的能量和功率性能.
- 确定液化工艺的低效率和需要改进的领域.
主要方法:
- 使用Aspen HYSYS V12对三个液化循环的模拟和分析.
- 评估每个周期的能量和功率效率,包括冷却前和冷却后阶段.
- 具体能源消耗,性能系数 (COP) 和整体能量效率 (EXE) 的比较.
主要成果:
- 循环3显示了最高的冷却前功率效率 (61.21%) 和最低的功率损失 (19.73%).
- 在冷冷却过程中,这三个周期都表现出超过50%的显著能量损失.
- 具体能源消耗在6.601至6.618MJ/kg之间,COP值约为0.199和EXE值接近45.8%,具体能源消耗在6.601至6.618MJ/kg之间.
结论:
- 第三个循环的设计显示了在冷却前阶段提高了能量利用率.
- 冷却仍然是提高液化效率的一个主要领域.
- 详细的热力学分析对于优化液化循环和推进清洁能源技术至关重要.
相关概念视频
Reduction of Alkenes: Catalytic Hydrogenation
11.9K
Alkenes undergo reduction by the addition of molecular hydrogen to give alkanes. Because the process generally occurs in the presence of a transition-metal catalyst, the reaction is called catalytic hydrogenation.
Metals like palladium, platinum, and nickel are commonly used in their solid forms — fine powder on an inert surface. As these catalysts remain insoluble in the reaction mixture, they are referred to as heterogeneous catalysts.
The hydrogenation process takes place on the...
Metals like palladium, platinum, and nickel are commonly used in their solid forms — fine powder on an inert surface. As these catalysts remain insoluble in the reaction mixture, they are referred to as heterogeneous catalysts.
The hydrogenation process takes place on the...
11.9K
The Carnot Cycle
2.8K
Converting work to heat is an irreversible process, and the purpose of a heat engine is to reverse the effect partially. Heat engines aim to increase the efficiency of the reversal, that is, maximize the work retrieved from heat. If the efficiency of a heat engine were 100%, it would imply reversing the process completely without introducing any other effect. Thus, it would violate the second law of thermodynamics.
What could be the theoretical limit to the efficiency of a heat engine? The...
What could be the theoretical limit to the efficiency of a heat engine? The...
2.8K
Hess's Law
44.7K
There are two ways to determine the amount of heat involved in a chemical change: measure it experimentally, or calculate it from other experimentally determined enthalpy changes. Some reactions are difficult, if not impossible, to investigate and make accurate measurements for experimentally. And even when a reaction is not hard to perform or measure, it is convenient to be able to determine the heat involved in a reaction without having to perform an experiment.
44.7K
Free Energy Changes for Nonstandard States
11.1K
The free energy change for a process taking place with reactants and products present under nonstandard conditions (pressures other than 1 bar; concentrations other than 1 M) is related to the standard free energy change according to this equation:
where R is the gas constant (8.314 J/K·mol), T is the absolute temperature in kelvin, and Q is the reaction quotient. This equation may be used to predict the spontaneity of a process under any given set of conditions.
Reaction Quotient...
where R is the gas constant (8.314 J/K·mol), T is the absolute temperature in kelvin, and Q is the reaction quotient. This equation may be used to predict the spontaneity of a process under any given set of conditions.
Reaction Quotient...
11.1K
Thermochemical Equations
28.3K
For a chemical reaction (the system) carried out at constant pressure – with the only work done caused by expansion or contraction – the enthalpy of reaction (also called the heat of reaction, ΔHrxn) is equal to the heat exchanged with the surroundings (qp).
28.3K
Efficiency of The Carnot Cycle
2.5K
The hypothetical Carnot cycle consists of an ideal gas subjected to two isothermal and two adiabatic processes. Since the internal energy of an ideal gas depends only on its temperature, which is the same before and after the completion of the Carnot cycle, there is no change in its internal energy. Hence, using the first law of thermodynamics, the total heat exchanged by the ideal gas equals the total work done. Thus, we can quantify the efficiency of the Carnot cycle via the heat exchanged...
2.5K


