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在八二年高考的化学试题里有这样一道题,综合其题意为:在25℃,容积为2升的容器里,反应 N_2 O_4(?)2NO_2-13.6千卡达到平衡后,改变影响平衡的一个条件,增加 N_2 O_4 的浓度摩尔比NO_2/N_2 O_4 怎样变化?(注:该题是试卷里第八题的最末一个小题)面对这样一道有相当难度的题目应怎样解答呢?有的认为,摩尔比“增大”。这显然是错误的。这是由于只考虑了增加 N_2 O_4浓度,平衡向右移动,造成 NO_2 浓度比原来平衡时增大而简单得出的错误结论。事
In the chemistry test of the college entrance examination in 1982, there was such a question, and its comprehensive meaning was: In a container with a capacity of 2 litres at 25°C, after the reaction N 2 O 4 (?) 2NO 2 -13.6 kcal reached equilibrium, the influence balance was changed. One condition is to increase the molar ratio of N_2O_4 to NO_2/N_2O_4 (Note: This question is the last question of the eighth question in the test paper.) How to solve the problem of such a difficult problem? Some think that the molar ratio “increases”. This is obviously wrong. This is due to the fact that only considering increasing the concentration of N 2 O 4 , the equilibrium shifts to the right, resulting in an erroneous conclusion that the concentration of NO 2 is larger than that of the original equilibrium. thing