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For the reaction N2 + 3H2 2NH3, the rate d[NH3]/dt = 2x10-4 Ms-1 .Therefore, the rate -d[N2]/dt is given as:
(a) -d[N2]/dt = 1/2d[NH3]/dt
If 'I' is the intensity of absorbed light and 'c' is the concentration of AB for the photochemical process AB + hv→ AB *, the rate of formation of AB * is directly proportional to:
(b) In photo initiated primary process rate of reaction is directly proportional to intensity of light used.
In a reaction, the rate expression is, rate = K[A][B]2/3[C]0 , the order of reaction is:
(c) Order of reaction is sum of powers raised on concentration terms in order to write rate expression.
The rate of a reaction get doubles when the temperature changes from 7°C to 17°C. By what factor will it change for the temperature change from 17°C to 27°C?
For the elementary step,
(CH3)3.CBr(aq) → (CH3)3C+ (aq) + Br- (aq) the molecularity is:
(b) Molecularity represents the number of molecules of reactants taking part in an elementary step of reaction.
The rate of disappearance of SO2 in the reaction; 2S02 +02 → 2S03 is 1.28 x10-3g/sec. Then the rate of formation of SO3 is:
(d) Rate of formation of SO3 = rate of disappearence of SO2
= 1.28x10-3 g/sec = 1.28x10-3/64 M/sec (64 is the molecular weight of SO2)
= (1.28x10-3/64)x80 g/sec = 1.60x10-3 g/sec
When ethyl acetate was hydrolysed in pressure of 0.1 N HCl, the rate constant was found to be 5.40 x 10-5 sec-1 . But when 0.1 N H2SO4 was used for hydrolysis, the rate constant was found to be 6.25 X10-5sec-1. Thus, it may be concluded that:
(a) Relative strength in favour of H2SO4 = rate constant of reaction catalysed by H2SO4 / rate constant of reaction catalysed by HCl
The half time of a second order reaction is:
(b) For II order reaction, t1/2 = 1/Ka
The rate constant of a second order reaction is 10-2 mol-1 litre s-1 The rate constant expressed in cc molecule-1min-1 is:
(a) K = 10-2mol-1litresec-1
= 10-2x1000x60/6.02x1023 cc molecule-1min-1
= 9.9618 x 10-22 cc molecule-1min-1
The half-life period of a first order chemical reaction is 6.93 minutes. The time required for the completion of 99% of the chemical reaction will be (log 2 = 0.301):
(b) t= (2.303x6.93/0.693)log(100/1)(N0 = 100; N = 100-99 =1)
t = 46.06 minute
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