Not sure if K_1[NO_2]^2 is correct for the production of CO_2, but I think it is
ID: 545918 • Letter: N
Question
Not sure if K_1[NO_2]^2 is correct for the production of CO_2, but I think it is the rate law for it. Can anyone do the steps to outline where I have gone wrong? I get another weird answer by using steady state conditions in a different method.
No,(g) + CO(g) co,(g) + NO(g) is suggested to be (1) 2NO2(g) NO,(g) + NO(g) k. (2) No,(g) + CO(g) NO2(g) + CO2(g) Assuming that [NO3l is governed by steady-state conditions, derive the rate law for the production of CO2(g) and enter it in the space below. rate of cOzg) productions[NO]Explanation / Answer
There are two step methods
Use the steady-state approximation to derive the rate law.
Production rate of NO3 = k1 [NO2]2
Consumption rate of NO3 = k2 [NO3] [CO]
A steady-state approach makes use of the assumption that the rate of production of an intermediate is equal to the rate of its consumption. Thus, we have
k1 [NO2]2 = k2 [NO3] [CO]
k2 = k1 [NO2]2 / [NO3] [CO]
rate of production of CO2 depends on NO3 production and consumption.
Related Questions
drjack9650@gmail.com
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.