Question

Given the following reaction: 2N2O5=2N2O4+O2, if the rate of oxygen production is 0.15M/min, determine:

a. The rate that N2O5 is consumed
b. The rate that N2O4 is produced

Answer 1

a.
`r_(N_2O_5)=-0.075M/min`

b.
`r_(N_2O_4)=0.075M/min`

Step-by-step explanation:

Hello.

In this case, according to the balanced chemical reaction, we can write the law of rate proportions:

`(r_(N_2O_5))/(-2) =(r_(N_2O_4))/(2) =(r_(O_2))/(1)`

Thus, we proceed as follows:

a. Since the rate of oxygen production is 0.15 M/min, we can make the following setup:

`(r_(N_2O_5))/(-2) =(r_(O_2))/(1)\\\\r_(N_2O_5)=(r_(O_2))/(-2) =(0.15M/min)/(-2)\\\\ r_(N_2O_5)=-0.075M/min`

b. Since the rate of oxygen production is 0.15 M/min, we can make the following setup:

`(r_(N_2O_4))/(2) =(r_(O_2))/(1)\\\\r_(N_2O_4)=(r_(O_2))/(2) =(0.15M/min)/(2)\\\\ r_(N_2O_4)=0.075M/min`

Best regards!