For a first order reaction A ⟶ B the rate constant is x min⁻¹. If the initial concentration of A is 0.01M, the concentration of A after one hour is given by the expression.

(a)

001. e^−x

(b)

1 x 10^-2(1-e^-60x)

(c)

(1 x 10^-2)e^-60x

(d)

none of these

A zero order reaction X ⟶ Product, with an initial concentration 0.02M has a half life of 10 min. if one starts with concentration 0.04M, then the half life is

(a)

10 s

(b)

5 min

(c)

20 min

(d)

cannot be predicted using the given information

Among the following graphs showing variation of rate constant with temperature (T) for a reaction, the one that exhibits Arrhenius behavior over the entire temperature range is _______.

(a)

(b)

(c)

(d)

both (b) and (c)

For a first order reaction A ⟶ product with initial concentration x mol L^-1, has a half life period of 2.5 hours. For the same reaction with initial concentration \(\left( \frac { x }{ 2 } \right) \) mol L^-1 the half life is

(a)

(2.5 x 2) hours

(b)

\(\left( \frac { 2.5 }{ 2 } \right) \) hours

(c)

2.5 hours

(d)

Without knowing the rate constant, t_1/2 cannot be determined from the given data

For the reaction, 2NH₃ ⟶ N₂ + 3H₂, if \(\frac { -d[NH_{ 3 }] }{ dt } \) = k₁[NH₃], \(\frac { d[N_{ 2 }] }{ dt } =k_{ 2 }[NH_{ 3 }],\frac { d[{ H }_{ 2 }] }{ dt } \)= k₃[NH₃] then the relation between k₁, k₂ and k₃ is _________.

(a)

k₁ = k₂ = k₃

(b)

k₁ = 3k₂ = 2k₃

(c)

1.5k₁ = 3k₂ = k₃

(d)

2k₁ = k₂ = 3k₃

The decomposition of phosphine (PH₃) on tungsten at low pressure is a first order reaction. It is because the _____.

(a)

rate is proportional to the surface coverage

(b)

rate is inversely proportional to the surface coverage

(c)

rate is independent of the surface coverage

(d)

rate of decomposition is slow

For a reaction Rate = k[acetone]^3/2 then unit of rate constant and rate of reaction respectively is _______.

(a)

(mol L^-1 S^-1),(mol^1/2 L^1/2 S^-1)

(b)

(mol^-1/2 L^1/2 s^-1),(mol L^-1 s^-1)

(c)

(mol^1/2 L^1/2 s^-1),(mol L^-1 s^-1)

(d)

(mol L s^-1),(mol^1/2 L^1/2 s)

The addition of a catalyst during a chemical reaction alters which of the following quantities?

(a)

Enthalpy

(b)

Activation energy

(c)

Entropy

(d)

Internal energy

Consider the following statements:
(i) increase in concentration of the reactant increases the rate of a zero order reaction.
(ii) rate constant k is equal to collision frequency A if E_a = 0
(iii) rate constant k is equal to collision frequency A if E_a = ∞
(iv) a plot of ln (k) vs T is a straight line.
(v) a plot of ln (k) vs \(\left( \frac { 1 }{ T } \right) \) is a straight line with a positive slope.
Correct statements are

(a)

(ii) only

(b)

(ii) and (iv)

(c)

(ii) and (v)

(d)

(i), (ii) and (v)

In a reversible reaction, the enthalpy change and the activation energy in the forward direction are respectively −x kJ mol^-1 and y kJ mol^-1. Therefore, the energy of activation in the backward direction is _______.

(a)

(y-x) kJ mol^-1

(b)

(x+y) J mol^-1

(c)

(x-y) KJ mol^-1

(d)

(x+y) x 10³J mol^-1

What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200K to 400K? (R = 8.314 JK^-1 mol^-1)

(a)

234.65 kJ mol^-1

(b)

434.65 kJ mol^-1 

(c)

2.305 kJ mol^-1 

(d)

334.65 J mol^-1

For a first order reaction, the rate constant is 6.909 min^-1 the time taken for 75% conversion in minutes is _______.

(a)

\(\left( \frac { 3 }{ 2 } \right) { \log 2 }\)

(b)

\(\left( \frac { 2 }{ 3 } \right) \log2\)

(c)

\(\left( \frac { 3 }{ 2 } \right) \log\left( \frac { 3 }{ 4 } \right) \)

(d)

\(\left( \frac { 2 }{ 3 } \right) \log\left( \frac { 4 }{ 3 } \right) \)

In a first order reaction x ⟶ y; if k is the rate constant and the initial concentration of the reactant x is 0.1M, then, the half life is_____.

(a)

\(\left( \frac { \log2 }{ k } \right) \)

(b)

\(\left( \frac { 0.693 }{ (0.1)k } \right) \)

(c)

\(\left( \frac { In2 }{ k } \right) \)

(d)

none of these

Predict the rate law of the following reaction based on the data given below 
2A+B⟶C+3D

Reaction number	[A] (min)	[B] (min)	Initial rate (M s-1)
1	0.1	0.1	x
2	0.2	0.1	2x
3	0.1	0.2	4x
4	0.2	0.2	8x

(a)

rate = k[A]² [B]

(b)

rate = k[A] [B]²

(c)

rate = k[A] [B]

(d)

rate = k[A]^1/2 [B]^3/2

The rate constant of a reaction is 5.8 x 10^-2  S^{​​​​​​-1} The order of the reaction is ______.

(a)

First order

(b)

zero order

(c)

Second order

(d)

Third order

For the reaction \({ N }_{ 2 }{ O }_{ 5 }\left( g \right) \longrightarrow { 2NO }_{ 2 }\left( g \right) +\frac { 1 }{ 2 } { O }_{ 2 }\left( g \right) \) value of rate of disappearance of N₂O₅ is given as 6.5 x 10^-2 mol L^-1s^-1. The rate of formation of NO₂ and O₂ is given respectively as_____.

(a)

(3.25 x 10^-2 mol L^-1s^-1) and (1.3 x 10^-2 mol L^-1s^-1) 

(b)

(1.3 x 10^-2 mol L^-1s^-1) and (3.25 x 10^-2 mol L^-1s^-1)

(c)

(1.3 x 10^-1 mol L^-1s^-1) and (3.25 x 10^-2 mol L^-1s^-1)

(d)

None of these

During the decomposition of H₂O₂ to give dioxygen, 48 g O₂ is formed per minute at certain point of time. The rate of formation of water at this point is

(a)

0.75 mol min⁻¹

(b)

1.5 mol min⁻¹

(c)

2.25 mol min⁻¹

(d)

3.0 mol min⁻¹

If the initial concentration of the reactant is doubled, the time for half reaction is also doubled. Then the order of the reaction is______.

(a)

Zero

(b)

one

(c)

Fraction

(d)

none

In a homogeneous reaction A⟶B+C+D, the initial pressure was P₀ and after time t it was P expression for rate constant in terms of P₀, P and t will be _____.

(a)

\(k=\left( \frac { 2.303 }{ t } \right) \log\left( \frac { 2{ P }_{ 0 } }{ { 3P }_{ 0 }-P } \right) \)

(b)

\(k=\left( \frac { 2.303 }{ t } \right) \log\left( \frac { { 2P }_{ 0 } }{ { P }_{ 0 }-P } \right) \)

(c)

\(k=\left( \frac { 2.303 }{ t } \right) \log\left( \frac { 3{ P }_{ 0 }-P }{ 2P_{ 0 } } \right) \)

(d)

\(k=\left( \frac { 2.303 }{ t } \right) \log\left( \frac { 2{ P }_{ 0 } }{ { 3P }_{ 0 }-2P } \right) \)

 If 75% of a first order reaction was completed in 60 minutes, 50% of the same reaction under the same conditions would be completed in_______.

(a)

20 minutes

(b)

30 minutes

(c)

35 minutes

(d)

75 minutes

The half life period of a radioactive element is 140 days. After 560 days, 1 g of element will be reduced to

(a)

\(\left( \frac { 1 }{ 2 } \right) g\)

(b)

\(\left( \frac { 1 }{ 4 } \right) g\)

(c)

\(\left( \frac { 1 }{ 8 } \right) g\)

(d)

\(\left( \frac { 1 }{ 16 } \right) g\)

The correct difference between first and second order reactions is that________.

(a)

A first order reaction can be catalysed; a second order reaction cannot be catalysed.

(b)

The half life of a first order reaction does not depend on [A₀]; the half life of a second order reaction does depend on [A₀].

(c)

The rate of a first order reaction does not depend on reactant concentrations; the rate of a second order reaction does depend on reactant concentrations.

(d)

The rate of a first order reaction does depend on reactant concentrations; the rate of a second order reaction does not depend on reactant concentrations.

After 2 hours, a radioactive substance becomes \(\left( \frac { 1 }{ 16 } \right) ^{ th }\) of original amount Then the half life (in min) is _______.

(a)

60 minutes

(b)

120 minutes

(c)

30 minutes

(d)

15 minutes

This reaction follows first order kinetics. The rate constant at particular temperature is 2.303 x 10^-2 hour^-1. The initial concentration of cyclopropane is 0.25 M. What will be the concentration of cyclopropane after 1806 minutes? (log 2 = 0.3010)

(a)

0.125 M

(b)

0.215 M

(c)

0.25 x 2.303 M

(d)

0.05 M