Nitrogen monoxide reacts with chlorine gas according to the following equation.

Question

Nitrogen monoxide reacts with chlorine gas according to the following equation.

2NO(g) + Cl2(g) ---> 2NOCl(g)

This reaction is second order in [?NO] and first order in [Cl2?]. If the rate constant at a particular temperature is 180 M??2 s?1, what is d?[?NOCl]?/?dt when the initial concentration of NO is 0.35 M and the initial concentration of Cl2is 0.15 M?

(A) 3.3 M?/?s

(B) 6.6 M?/?s

(C) 19 M?/?s

(D) 38 M?/?s

Since there are 2 moles of NOCL, wouldn't you double the answer to get 6.6? Why or why not?

Explanation / Answer

rate = K3 [NO]^2[Cl2]^1

rate = 180 *(0.35)^2(0.15)^1

rate = 3.307 M/sec

as per the above chemical eq.

we can write

rate = +1/2[NO] = [Cl2] = - 1/2 [NOCl]

so

rate = -1/2[NOCl]

[NOCl] = -2*3.307 = 6.6 M/se

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