Chlorine gas reacts with carbon monoxide to produce phosgene according to the fo

Question

Chlorine gas reacts with carbon monoxide to produce phosgene according to the following chemical reaction: Cl2(g) + CO(g) right arrow Cl2C0(g) It is experimentally observed that when the concentration of CO is decreased 10-fold, the rate of the reaction also decreases by a factor of 10, while when the concentration of Cl2 is increased 10-fold, the rate of the reaction increases by approximately a factor of 30. a) Write down the rate law for this reaction in terms of a rate constant, k, and the concentrations of Cl2 and CO. b) What is the overall order of the reaction, and the orders with respect to Cl2 and CO? c) What are the units of k for the reaction? d) If the rate of the reaction at time t is equal to u, and the concentrations of Cl2 and CO are instantaneously increased by a factor of 2 and 3, respectively, what is the reaction rate in units of u.

Explanation / Answer

Rate of reaction =k [Cl2]x[CO]y ..........1

let initial concentrations of Cl2 and CO are A and B.

if concentartion of CO decreased by 10 fold then concentarion of CO = B/10

when  CO decreased by 10 fold then rate of reaction decreases by factor 10.

keeping all values ;

R/10 =k [A]x[B/10]y ..............2

divide 2 nad 1 implies

1/10 = [1/10]y

implies y =1

when Cl2 increased by 10 times, rate is increased by 30 times implies ===>

30R =k [10A]x[B] ..................3 [since y=1]

dividing 3 and 1

30 = 10x

x = 1.5 [approximately]

a] Rate of reaction =k [Cl2]1.5[CO]1

b]Overall order is 2.5

with respect to Cl2 is 1.5

with respect to CO is 1

c] k = ML2.5/(tM2.5*L) ===> L1.5 S-1M-1.5   [L = litre ; M = mole ; s = sec]

d] rate of reaction initial is V

Cl2 and CO increase by a factor of 2 and 3 then

keeping all values

Rate of reaction = 8.485 V = 8.5V approximatley

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