The reaction

2HNO2(g) → H2O(g) + NO(g) + NO2(g)

is second order in HNO2(g) and has a rate constant of 6.03 L·mol–1·s–1. If a reaction mixture is initially 0.0681 mol·L–1 in HNO2(g), what is the concentration of HNO2(g) after 234 s?

Question

The reaction

2HNO2(g) → H2O(g) + NO(g) + NO2(g)

is second order in HNO2(g) and has a rate constant of 6.03 L·mol–1·s–1. If a reaction mixture is initially 0.0681 mol·L–1 in HNO2(g), what is the concentration of HNO2(g) after 234 s?

BlackTom AI · Accepted Answer

The problem presents a second-order reaction: 2HNO2(g) → products, with rate law for a second-order reaction depending on the concentration of HNO2: rate = k [HNO2]^2.

For a second-order reaction in A, the integrated rate law is: 1/[A] = 1/[A]0 + kt, where [A]0 is the initial concentration, t is time, and k is the rate constant.

Given data:
- [HNO2]0 = 0.0681 M
- k = 6.03 L·mol–1·s–1
- t = 234 s

Calculate 1/[A]:
- Compute 1/[A]0 = 1 / 0.0681 ≈ 14.7 (units: L·mol–1)
- Compute kt = (6.03) × (234) ≈ 1411.02
- Sum: 1/[A] = 14.7 + 1411.02 ≈ 1425.72

Now invert to get [A]:
- [HNO2] = 1 / 1425.72 ≈ 7.01 × 10^–4 M

Thus, the concentration of HNO2 after 234 s is approximately 7.01 × 10^–4 mol·L–1.

Note on options: The provided answer is a single option: 7.01 × 10^–4 mol·L–1. Since there were no other options listed to evaluate, this calculation directly confirms that the given value matches the correct application of the second-order integrated rate law with the supplied k, initial concentration, and time.

The reaction 2HNO2(g) → H2O(g) + NO(g) + NO2(g) is second order in HNO2(g) and has a rate constant of 6.03 L·mol–1·s–1. If a reaction mixture is initially 0.0681 mol·L–1 in HNO2(g), what is the concentration of HNO2(g) after 234 s?单项选择题

类似问题

The half-life for the second-order decomposition of a drug is 52 min. Find the time required for the 30% decomposition reaction. Report your answer in whole minutes.

A drug with concentration 0.70 M decomposes via acid-catalysed hydrolysis with a rate constant of 0.013 M−1 h−1. What is the drug concentration after 61 hours? Report your answer to 2 decimal places.

What are the units of the rate constant k for a second-order reaction?

The half-life for the second-order decomposition of HI is 15.4 s when the initial concentration of HI is 0.34 M. What is the rate constant for this reaction?

Consider the chemical reaction of the type 2A → P, that reacts with second order kinetics. Identify which of the following statements is correct.

The reaction 2NO3(g) → 2NO2(g) + O2(g) has the rate law: rate = k[NO3]2. The half-life for the reaction is 53.5 s when the initial concentration of NO3 is 0.845 M. Calculate the time needed for the concentration of NO3 to decrease to one-fourth of its original value.

The reaction 2HNO2(g) → H2O(g) + NO(g) + NO2(g) is second order in HNO2(g) and has a rate constant of 6.03 L·mol–1·s–1. If a reaction mixture is initially 0.0681 mol·L–1 in HNO2(g), what is the concentration of HNO2(g) after 234 s?

更多留学生实用工具

智能学习助手

风格化写作助手

论文查重助手

文献引用助手

课堂转译助手

课堂笔记助手

Quiz搜索助手

学校历年真题

智能刷题助手

智能匹配练习

希望你的学习变得更简单