Consider the following reaction: 2{/rm{ N}}_2 {/rm{O (}}g) /; / rightarrow /; 2{/rm{ N}}_2 (g) /; + /; {/rm{O}}_2 (g)

a. In the first 12.0 s of the reaction, 1.7*10-2 mol of {/rm{O}}_2 is produced in a reaction vessel with a volume of 0.240 L. What is the average rate of the reaction over this time interval?

b. Predict the rate of change in the concentration of {/rm{N}}_2 {/rm{O}} over this time interval. In other words, what is {/Delta [{/rm{N}}_2 {/rm{O}}]}/{/Delta t}?

Question

Chemistry

Clinton Villanueva

25 November, 01:48

Consider the following reaction: 2{/rm{ N}}_2 {/rm{O (}}g) /; / rightarrow /; 2{/rm{ N}}_2 (g) /; + /; {/rm{O}}_2 (g)

a. In the first 12.0 s of the reaction, 1.7*10-2 mol of {/rm{O}}_2 is produced in a reaction vessel with a volume of 0.240 L. What is the average rate of the reaction over this time interval?

b. Predict the rate of change in the concentration of {/rm{N}}_2 {/rm{O}} over this time interval. In other words, what is {/Delta [{/rm{N}}_2 {/rm{O}}]}/{/Delta t}?

+2

Answers (1)

Know the Answer?

Jordyn Clayton · Answer 1

a. 5.9 * 10⁻³ M/s

b. 0.012 M/s

Explanation:

Let's consider the following reaction.

2 N₂O (g) → 2 N₂ (g) + O₂ (g)

a.

Time (t) : 12.0 s

Δn (O₂) : 1.7 * 10⁻² mol

Volume (V) : 0.240 L

We can find the average rate of the reaction over this time interval using the following expression.

r = Δn (O₂) / V * t

r = 1.7 * 10⁻² mol / 0.240 L * 12.0 s

r = 5.9 * 10⁻³ M/s

b. The molar ratio of N₂O to O₂ is 2:1. The rate of change of N₂O is:

5.9 * 10⁻³ mol O₂/L. s * (2 mol N₂O/1 mol O₂) = 0.012 M/s