I.For the reaction: 2 NO (g) +O2(g)- 2 NO2 (g). gi ven the following data determ
ID: 716821 • Letter: I
Question
I.For the reaction: 2 NO (g) +O2(g)- 2 NO2 (g). gi ven the following data determine the rate law and the rate constant (with correct units). Exp # 02 e (M/s) .0040 55.6 2. For the reaction: 2A + B disappearance of A and the rate of appearance of C? 3 the rate of disappearance of B was 0.30 M/s. What is the rate of The decompoosition reaction: SO Cl2SO2+Cl2, has a first order rate constant of 2.2x10-ss-1 at 3200. If the initial concentration of SO Cl2 is 0.0040 M, what will be its concentration be (a) after 1.00 hr and (b) after 1.00 day? 3. The decomposition reaction 2 HI (g) H2 (g) + 12 (g), is second order and has a rte constant equal to 1.6 x 103 M. is' at 700 °C. If the initial concentration of HI in the container is 3.4 x 10-2 M, how many minutes will it take for the concentration to be reduced to 8.0 x 10 M? The conversion of cyclopropane to propylene is first order and has a rate constant of 1.3 x 10 s at 400 °C The rate constant is 1.1 x 10 s at 430 °C. What is the activation energy in kJ/molt?Explanation / Answer
Q1;
2NO(g) + O2 (g) -----> 2NO2(g)
Let order w.r.t. NO is x and rate w.r.t. O2 is y
Rate = k [NO]x [O2]y
From Exp No. 1
7.10 = k [0.001]x [0.001]y ------(1)
k = rate constant
From Exp 2
28.4 = k [0.004][0.001] ----------(2)
Divide (2) by (1)
28.4 / 7.1 = k [0.004]x [0.001]y / k [0.001]x [0.001]y
4 = 4x
Hence x = 1
On similar bases as above, from Exp no. 2 and 3 it can be shown that
255.6 / 28.4 = k [0.004]x [0.003]y / k [0.004]x [0.001]y
9 = 3y
Hence y = 3
Thus the rae law of the reaction is:
Rate = k [NO] [O2]3