Consider the reaction,

2AsH3(g) → 2As(g) + 3H2(g)

If the rate of formation of H2(g) is 0.090 mol·L—1·s—1, then the rate of formation of of As(g) is:

Question

Consider the reaction,

2AsH3(g)  →  2As(g) + 3H2(g)

If the rate of formation of H2(g) is 0.090 mol·L—1·s—1, then the rate of formation of of As(g) is:

BlackTom AI · Accepted Answer

The question presents the balanced chemical equation: 2AsH3(g) → 2As(g) + 3H2(g). To relate the rates, use the stoichiometric coefficients: for every 3 moles of H2 formed, 2 moles of As are formed.

Option 1: 0.030 mol·L—1·s—1. If you compare to the given rate of H2 formation (0.090), this option would imply a conversion factor of 0.030/0.090 = 1/3, which does not match the 3:2 ratio between H2 and As formation. Therefore this is inconsistent with the stoichiometry.

Option 2: 0.045 mol·L—1·s—1. This corresponds to a 0.045/0.090 = 1/2 ratio. The reaction shows a 3:2 ratio between H2 and As formation, not 1:2, so this option misuses the stoichiometric relationship.

Option 3: 0.060 mol·L—1·s—1. Here, 0.060/0.090 = 2/3. This exactly reflects the 2 moles of As formed per 3 moles of H2 produced in the balanced equation. The rate of formation of As(g) should be (2/3) times the rate of H2 formation, which computes to 0.060.

Option 4: 0.090 mol·L—1·s—1. This would imply the same rate as H2 formation, which would correspond to a 1:1 relationship. The stoichiometry does not support equal rates for H2 and As formation, since three hydrogens are produced for every two arsenic atoms formed.

Option 5: 0.135 mol·L—1·s—1. This would be more than the given H2 rate by a factor of 1.5, which again contradicts the 3:2 stoichiometric ratio and overshoots the expected rate based on the reaction coefficients.

In summary, the only option that aligns with the reaction’s 3 H2 produced for every 2 As formed is the one where the rate of As formation is (2/3) times the rate of H2 formation, yielding 0.060 mol·L—1·s—1.

Consider the reaction, 2AsH3(g) → 2As(g) + 3H2(g) If the rate of formation of H2(g) is 0.090 mol·L—1·s—1, then the rate of formation of of As(g) is:

查看解析

登录即可查看完整答案

类似问题

Reaction rates have units of .

Given the following balanced equation, determine the rate of reaction with respect to [HCl]. H2(g) + Cl2(g) → 2 HCl(g)

According to the following reaction, disappearance rate of oxygen is 5.75 x 10-2 mol L-1 s-1. Determine formation rate of dinitrogen pentaoxide (g)? 4 NO2(g) + O2(g) → 2 N2O5(g)

The average rate of disappearance of ethane (C2H6) in the reaction, 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(g) is found to be 1.50 × 10–3 M·s–1 over a certain interval of time. What is the rate of appearance of H2O during this time interval?

The rate of disappearance of N2O5 is 3.6 x 10−4 M/s in the reaction below. What is the rate of appearance of NO2? 2 N2O5 → 4 NO2 + O2

If at a certain instant during the course of the reaction, 2NO2(g) + F2(g) → 2NO2F(g) the rate of the formation of the product were 0.16 mol·L–1·s–1, how fast would the F2(g) be disappearing (also in mol·L–1·s–1) at that same instant in time?

Consider the reaction: 4NO2 + O2 → 2N2O5 If N2O5 is being produced at a rate of 1.2 x 10-4 M/s, what is the rate at which NO2 is being consumed, in mol/(L.s)?

The rate of a reaction:

更多留学生实用工具

考试浏览器助手

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