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330
*22.
What is the order for the following reactions?
(a) 2NO 2 (g) + F2 (g) ⎯⎯
→ 2NO 2 F (g) , rate = k[NO2][F2]
(b) CHCl 3 (g) + Cl 2 (g) ⎯⎯
→ CCl 4 (g) + HCl(g) , rate = k[CHCl 3 ] [Cl 2
Ans.
(a) 2NO 2 (g) + F2 (g) ⎯⎯
→ 2NO 2 F (g) , rate = k[NO2][F2]
∴ Order = 1 + 1 = 2
(b) CHCl 3 (g) + Cl 2 (g) ⎯⎯
→ CCl 4 (g) + HCl(g) , rate = k[CHCl 3 ] [Cl 2
∴ Order = 1 +
*23.
Ans.
*24.
1
]2
1
]2
1
3
=
2
2
Write the rate law for the following reactions :
(a) A reaction that is zero order in A and second order in B.
(b) A reaction that is second order in NO and first order in Br2.
(a) If the reaction is zero order in A and second order is B
Then, Rate = k [A]0 [B]2
Rate = k [B]2.
(b) If the reaction is 2nd order in NO and first order in Br2, then Rate = k[NO]2[Br]1.
Consider the reaction
Tl + (aq) + 2Ce 4+ (aq) ⎯⎯
→ Tl 3+ (aq) + 2Ce 3+ (aq) . The rate law for the reaction is rate = k
[Ce4+] [Mn2+]. In the presence of Mn2+ the reaction occurs in the following elementary steps :
(a) Ce 4+ (aq) + Mn 2+ (aq) ⎯⎯
→ Ce 3+ (aq) + Mn 3+ (aq)
(b) Ce 4+ (aq) + Mn 3+ (aq) ⎯⎯
→ Ce 3+ (aq) + Mn 4+ (aq)
(c) Tl + (aq) + Mn 4+ (aq) ⎯⎯
→ Tl 3+ (aq) + Mn 2+ (aq)
Ans.
Identify (a) catalyst (b) intermediate (c) rate determining step.
(a) The catalyst in the above reaction will be Mn+2. Since Mn+2 is present at the start as
well as end of the reactions.
(b) The intermediate in the above reaction will be Mn3+ and Mn4+ since both Mn+3 and Mn+4
are formed in one step and consumed is the next step.
(c) The rate law given is Rate = k[Ce4+] [Mn2+].
∴ The rate determining step will be Ce 4+ (aq) + Mn 2+ (aq) ⎯⎯
→ Ce +3 (aq) + Mn 3+ (aq) .
*25.
Ans.
Comment on the relationship between coefficients of the balanced overall equation for a reaction
and the exponents to which the concentration terms in the rate law are raised.
What do these exponents represent?
(a) The rate of a reaction at a given temperature depends on the concentration of reactants.
Unique Solutions ®
S.Y.J.C. Science - Chemistry - Part I
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