Consider the gas-phase reaction between nitric oxide and bromine at 273 degree C

Question

Consider the gas-phase reaction between nitric oxide and bromine at 273 degree C 2NO(g) + Br_2 (g) rightarrow 2NOBr(g). The following data for the initial rate of appearance of NOBr were obtained: Calculate the average value of the rate constant for the appearance of NOBr from the four data sets. Express your answer using two significant figures. How is the rate of appearance of NOBr related to the rate of disappearance of Br_2? the rate of appearance of NOBr is half the rate of disappearance of Br_2 the rate of disappearance of Br_2 is half the rate of appearance of NOBr the rate of disappearance of Br_2 is equal to the rate of appearance of NOBr What is the rate of disappearance of Br_2 when [NO] = 8.6 times 10^-2 M and [Br_2] = 0.23 M?

Explanation / Answer

D)
rate law is:
rate = k [NO]^2 * [Br2]

at given concentration,
rate = 1.2*10^4 * (8.6*10^-2)^2 * (0.23)
= 20.4 M/s
This is rate of appearance of NOBr

from Part C,
rate of disappearance of Br2 = 0.5*rate of appearance of NOBr
= 0.5*20.4 M/s
= 10.2 M/s

Answer: 10.2 M/s

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