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在一定温度下,一个化学反应平衡体系受总压改变的影响,平衡被破坏,体系将调整反应物和产物浓度值,重新建立平衡。对题述平衡体系增大(或减小)压力时,根据勒夏特列原理可以推断,重新建立平衡时,氨的浓度要增大(或减小)。而氮及氢的浓度变化情况较为复杂。本文对这个问题做一讨论。设某浓度时,理想气体反应体系N_(2(g))+3H_(2(g))→2NH_(3(g))在反应进度为ξ时达平衡;平衡体系中氮、氢及氨的物质的量分别为x(mol)、y(mol)及,z(m(?));平衡体系的体积力V(m~3);平衡体系中氮、氢及氨的浓度分别为[N_2](mol.m~(-3))、[H_2](mol.m~(-3))及[NH_3](mol.m~(-3));以浓
At a certain temperature, a chemical reaction equilibrium system is affected by the total pressure change, the balance is destroyed, the system will adjust the reactant and product concentration values, to re-establish the balance. When increasing (or decreasing) the pressure on the subject equilibrium system, it can be inferred from the Le Chatelier principle that the concentration of ammonia increases (or decreases) when equilibrium is re-established. The nitrogen and hydrogen concentration changes are more complicated. This article is a discussion of this issue. When a certain concentration is set, the ideal gas reaction system N 2 (g) + 3H 2 (g) → 2NH 3 (g) equilibrates when the reaction progress is ξ; the equilibrium nitrogen, hydrogen and ammonia The amount of material is respectively x (mol), y (mol) and z (m (?)); The volume force V (m ~ 3) of the equilibrium system; the concentration of nitrogen, hydrogen and ammonia in the equilibrium system are [N2 ] (mol.m ~ (-3)), [H_2] (mol.m -3) and [NH_3] (mol.m -3)