PLEASE HELP QUESTION 3 & 4 Questions 2 and 3 use the following data: NO2 (g) O3(

Question

PLEASE HELP QUESTION 3 & 4

Questions 2 and 3 use the following data: NO2 (g) O3(g) NO3 (g) o20g) [NO2]i (M) (M) Initial Rate (M-ls- l) [O3li 0.10 0.33 1.42 2.84 0.66 0.10 7.10 0.25 0.66 2. Determine the rate law Rate- k[NO2][O3] B) Rate- k[NO2][O3]2 3. The k value for the rale law constant. A) Rate 430 M-1 s-1 B) Rate 227 M-2s-1 Rate- 43 M-1s-1 4. The first-order decomposition rate constant is 6.7 x 10-4 s-1. If the initial concentration is 1.33 M, what is the concentration after 644 s? A) 0.43 M 86 M C) 0.94 M D) 0.15 M

Explanation / Answer

2.

Suppose rate law is:

R = k [NO2]a[O3]b

From experiment 1 and 2

1.42 = k (0.10)a x (0.33)b …………………(i)

2.84 = k (0.10)a x (0.66)b ………………(ii)

From equation (i) and (ii)

(2)b = 2

b = 1

From experiment 3

7.10 = k (0.25)a x [0.66]b ………………..(iii)

From equation (ii) and (iii)

7.10/2.84 = (0.25)a /(0.10)a

2.5 = (2.5)a

a = 1

Rate law:

Rate = k [NO2] [O3]

3.

1.42 = k (0.10)a x (0.33)b …………………(i)

1.42 = k (0.1)1(0.33)1

K = 43 M-1s-1

4. k = 2.303/t logN0/N

6.7 x 10-4 = 2.303/644 log 1.33/N

Log1.33/N = 1.873 x 10-1

Log1.33/N = log 1.5392

1.33/N = 1.5392

N = 0.86

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