题目
题目
单项选择题

Consider the tabulated data collected for the reaction 2N2O(g) → 2N2(g) + O2(g) at 500 °C. The rate law for this reaction is rate = k[N2O]. Time (s) [N2O] (M) 0 0.2400 61.9 0.1200 123.8 0.0600 185.7 0.0300 What is the value of the rate constant at this temperature?

选项
A.6.73 × 10–2 s–1
B.4.86 × 10–3 s–1
C.1.94 × 10–3 s–1
D.3.88 × 10–3 s–1
E.1.12 × 10–2 s–1
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标准答案
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思路分析
First, I restate the problem to ensure clarity: the reaction follows a rate law of rate = k[N2O], and from the data, [N2O] halves after each 61.9 s interval (0.2400 → 0.1200 → 0.0600 → 0.0300). This pattern indicates first-order decay with respect to N2O because a constant half-life across these successive intervals is a hallmark of first-order kinetics. Option 1: 6.7......Login to view full explanation

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