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STK 2023 PHYSICAL CHEMISTRY 2
ASSIGNMENT 1
Question 1 (a) Rate of formation = 13d[O2]dt
Rate of disappearance = - 12d[O3]dt

(b) Rate of formation = 12d[HF]dt = d[O2]dt
Rate of disappearance = - 12d[HOF]dt

(c) Rate of formation = 12d[BrNO]dt
Rate of disappearance = - 12d[NO]dt= - d[Br2]dt

Question 2
2NO(g) + H2(g) N2O(g) + H2O(g) (a) Rate = k[NO]2[H2] (b) 0.005 = k(0.075)2(0.400)
0.005 = k(2.25 x 10-3) k = 2.22 M-2 s-1

Question 3 Temperature (K) | Rate constant (M/s) | 1/T (K-1) | ln k | 573 | 2.91 x 10-6 | 0.00175 | -12.75 | 673 | 8.38 x 10-4 | 0.00149 | -7.08 | 773 | 7.65 x 10-2 | 0.00130 | -2.57 |

Plot of ln k against 1/T (K-1)

Slope of graph, m = -7.08-(-12.75)0.00149-0.00175 = 5.67- 0.00026 = 21807.69
Using Arrhenius equation, m = - Ea8.314 J/Kmol 21807.69 = - Ea8.314 J/Kmol Ea = 181 kJ/mol

Question 4 (a) Rate of reaction of NO is second order. Rate of reaction of H2 is first order. Total rate of reaction = third order. (b) If [NO] is doubled, the rate of reaction quadruples. (c) If [H2] is halved, the rate of reaction is halved.

Question 5
Initial concentration = Ao
Final concentration = A
Time, t = 65s – 45s = 20s
Use ln A = -kt + ln Ao ln (8.70 x 10-3M) = - (k)(20s) + ln (7.30 x 10-2M) -4.744 = - (k)(20s) + (-2.617) 2.127 = (k)(20s) k = 0.106 s-1

Question 6
The rate law is determined based on the slow reaction since the fast reactions are not in equilibrium.
∴ Rate = k[H2O2][I-]

Question 7 (a) Rate = k[A]m[B]n
Find m and n.
2 x 10-3 = k(0.10)m(0.10)n ------- (i)
8 x 10-3 = k(0.20)m(0.10)n ------- (ii)
(ii) ÷ (i)
4 = 2m
∴ m = 2

8.0 x 10-3 = k(0.20)m(0.10)n ------- (i)
8.0 x 10-3 = k(0.20)m(0.20)n ------- (ii)
(ii) ÷ (i)
1 = 2n
∴ n = 0

Rate = k[A]m[B]n = k[A]2[B]0 = k[A]2

(b) Rate = k[A]2
2 x 10-3 = k(0.10)2
2 x 10-3 = k(0.01)
∴ k = 0.2 M-1 s-1

(c) Step 1: A + B C + M (slow)
Step 2: M + A C (fast)

STK 2023 PHYSICAL CHEMISTRY 2
ASSIGNMENT 1

NAME | GLORIA AUGUSTA WILLIAM34855 | GROUP | 3 | LECTURER’S NAME | MDM AMIRA SATIRAWATY | DATE OF SUBMISSION | 1/4/2014 |

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