Answer the following questions related to the to kinetics of chemical reactions.

Question

Answer the following questions related to the to kinetics of chemical reactions. I^-(aq)+CIO^-(aq)oh-rightarrow IO^-(aq)=CI^-(aq) Iodie ion,I^-,is oxidized to hypoiodite ion IO^-, by hyopchlorite,CIO-,in basic solution according to equation above. Three initial-rate experiments were conducted; the results shown in the following table (a) Determine the order of the reaction with respect to each reactant listed below. Show your work. (i) I^-(aq) (ii) CIO^-(aq) (b) For the reaction, (i) write the rate law that is consistent with the calculations in part (a); (ii) calculate the value of the specific rate constantt, k, and specify units. The catalyzed decomposition of hydrogen peroxide, H_2O_2(aq), is represented by the following equation.

Explanation / Answer

Given reaction is I- + ClO- -----------> IO- + Cl-

rate = k [ I- ]m [ClO-]n    k = rate constant

From trial 1,

0.156 = k [0.017]m [0.015]n ------- Eq (1)

From trial 2,

0.476 = k [0.052]m [0.015]n --------Eq (2)

From trial 3,

0.596 = k [0.016]m [0.061]n --------Eq (3)

Do Eq(2)/Eq(1),

(0.476/0.156) = (k/k) (0.052/0.017)m (0.015/0.015)n

3.05 = 3.05m x 1n  

3.05 = 3.05m

Therefore, m =1

Do Eq(1)/Eq(3),

(0.156/0.596) = (k/k) (0.017/0.016)m (0.015/0.061)n

0.26 = (1.0625)m x (0.245)n

Substitute m=1,

0.26 = (1.0625)1 x (0.245)n

0.245 = (0.245)n

n= 1

Therefore, m= 1, n= 1

Hence,

rate = k [I-]1 [ClO-]1

i.e. rate = k [I-] [ClO-]

a) (i) order of reaction w.r.to I- = 1

(ii) order of reaction w.r.to ClO- = 1

b) (i)  Rate law is rate = k [I-] [ClO-]

(ii)

Use trail 1, to get the value of k

0.156 mol/L//s = k [0.017 mol/L] [0.015 mol/L]

k = 611.7 L mol-1 s-1

Therefore, specific rate constant k =  611.7 L mol-1 s-1

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