1. The rate of a chemical reaction can be expressed in terms of

(a) rate of consumption of catalyst

(b) rate of consumption of reactants only

(c) rate of cousumption of reac tants and formation of products both

(d) rate of formation of products only.

2. The rate of a reaction is expressed in the units

(a) \(\mathrm{L} \mathrm{mol}^{-1} \mathrm{I}^{-1}\)

(b) mol \(\mathrm{dm}^{-1} \mathrm{t}^{-1}\)

(c) Ms

(d) \(\mathrm{M}^{-1} \mathrm{~s}^{-1}\)

3. In the reaction \(A+3 B \longrightarrow 2 C\), the rate of formation of \(\mathrm{C}\) is

(a) the same as rate of consumption of \(A\).

(b) the same as the rate of consumption of \(B\)

(c) twice the rate of consumption of \(\mathrm{A}\)

(d) \(3 / 2\) times the rate of consumption of \(\mathrm{B}\).

4. The instantaneous rate of reaction \(2 \mathrm{~A}+\mathrm{B}-\mathrm{C}\). \(+3 \mathrm{D}\) is given by

(a) \(\frac{\mathrm{dA}}{\mathrm{dt}}\)

(b) \(\frac{1}{2} d \mathrm{dt}\)

(c) \(\frac{\mathrm{d}[\mathrm{B}]}{\mathrm{dt}}\)

(d) \(\frac{1}{3} \frac{\mathrm{L}[\mathrm{D}]}{\mathrm{dt}}\)

5. A reaction is first order with respect to reactant \(A\) and second order with respect to reactant \(B\). The rate law for the reaction is given by

(a) rate \(=\mathrm{k}[\mathrm{A}][\mathrm{B}]^2\)

(b) rate \(=[\mathrm{A}][\mathrm{B}]^2\)

(c) rate \(=\mathrm{k}[\mathrm{A}]]^2[\mathrm{~B}]\)

(d) rate \(=\mathrm{k}[\mathrm{A}]^0[\mathrm{~B}]^2\)

6. Molecularity of an elementary reaction

(a) may be zero

(b) is always integgrai

(c) may be semi-integral

(d) may be integral, fractional or zero.

7. The unit of rate constant for first order reaction is

(a) min-2

(b) 5

(c) \(\mathrm{s}^{-11}\)

(d) \(\min\)

8. The integrated rate equation for first order reaction \(A \longrightarrow\) products is given by

(a) \(k=\frac{2.303}{1}\left[\mathrm{ln}]\mathrm{[A_0]}/[A_3]\right.\)

(b) \(k={ }_1^1[\mathrm{l}: \mathrm{A}]\)

(c) \(k=\frac{2.303}{t} \log _{10} \frac{[A]_2}{[A]}\) (d) \(k=\frac{1}{t} \ln \frac{[A]_0}{[A]}\)

9. The half life of a first order reaction is \(30 \mathrm{~min}\) and the initial concentration of the reactant is 0.1 M. If the initial concentration of reactant is doubled, then the half life of the reaction will be

(a) \(1800 \mathrm{~s}\)

(b) 60 min

(c) \(15 \mathrm{~min}\)

(d) \(900 \mathrm{~s}\)

10. The slope of the straight line obtained by plotting rate versus concentration of reactant for a first order reaction is

(a) \(-\mathrm{k}\)

(b) \(-\mathrm{k} / 2.303\)

(c) \(\mathrm{k} / 2.303\)

(d) \(\mathrm{k}\)

11. The reaction between \(\mathrm{H}_2(\mathrm{~g})\) and \(\mathrm{ICI}(\mathrm{g})\) occurs in the following steps:

i) \(\mathrm{H}_2+\mathrm{ICI} \longrightarrow \mathrm{HI}+\mathrm{HCl}\)

ii) \(\mathrm{HI}+\mathrm{ICI} \longrightarrow \mathrm{I}_2+\mathrm{HCI}\)

The reaction intermediate in the reaction is

(a) \(\mathrm{HCl}\)

(b) \(\mathrm{HI}\)

(c) 12

(d) ICl

12. Consider the reaction

\(2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_2(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_2(\mathrm{~g})\). If \(\frac{\mathrm{d}\left[\mathrm{NO}_2\right]}{\mathrm{dt}}=\)

\(0.052 \mathrm{M} / \mathrm{s}\) then \(\frac{\mathrm{d}\left[\mathrm{O}_2\right]}{\mathrm{dt}}\) will be

(a) \(0.052 \mathrm{M} / \mathrm{s}\)

(b) \(0.114 \mathrm{M} / \mathrm{s}\)

(c) \(0.026 \mathrm{M} / \mathrm{s}\)

(d) \(-0.026 \mathrm{M} / \mathrm{s}\)

13. The rate of the first order reaction

\(A \longrightarrow\) products is \(0.01 \mathrm{M} / \mathrm{s}\), when reactant concentration is \(0.2 \mathrm{M}\). The rate constant for the reaction will be

(a) \(0.05 \mathrm{~s}^{-1}\)

(b) 0.05 min \(^{-11}\)

(c) \(0.1 \mathrm{~s}^{-1}\)

(d) \(0.015^{-1}\)

14. The rate constant of a reaction

(a) decreases with increasing \(E\),

(b) decreases with decreasing \(E\),

(c) is independent of \(E\),

(d) decreases with increasing temperature

15. The slope of a graph \(\ln [A]_{\mathrm{E}}\) versus \(t\) for a first order reaction is \(-2.5 \times 10^{-2} \mathrm{~s}^{-1}\). The rate constant for the reaction \(w\) ill be

(a) \(5.76 \times 10^{-1} \mathrm{~s}^{-1}\)

(b) \(1.086 \times 10^{-3} \mathrm{~s}^{-1}\)

(c) \(-2.5 \times 10^{-1} \mathrm{~s}^{-1}\)

(d) \(2.5 \times 10^{-3} \mathrm{~s}^{-1}\)

16. Acatalyst increases the rate of the reaction by

(a) increasing \(E_a\)

(b) increasing \(\mathrm{T}\)

(c) decreasing \(E_{\text {. }}\)

(d) decreasing \(\mathrm{T}\)

17. The formation of \(\mathrm{SO}_3\) from \(\mathrm{SO}_2\) and \(\mathrm{O}_2\) takes place in the following steps

i) \(2 \mathrm{SO}_2+2 \mathrm{NO}_2 \longrightarrow 2 \mathrm{SO}_3+2 \mathrm{NO}\)

ii) \(2 \mathrm{NO}+\mathrm{O}_2 \longrightarrow 2 \mathrm{NO}_2\)

(a) \(\mathrm{NO}_2\) is intermediate

(b) \(\mathrm{NO}^2\) is catalyst

(c) \(\mathrm{NO}_2\) is catalyst and \(\mathrm{NO}\) is intermediate

(d) \(\mathrm{NO}_{\text {is catalyst and }} \mathrm{NO}\) is intermediate.

28. The reaction \(\left.\mathrm{H}_2 \mathrm{O}_{2(\mathrm{~b})} \rightarrow \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}+\mid \mathrm{O}\right]_{(2)}\) is a

(a) first order raction

(b) second order reaction

(c) zero order reaction

(d) third order reaction

29. Which equation is correct for first order reactions?

(a) \(t_{1 / 2} \propto C^{-1}\)

(b) \(\mathrm{t}_{1 / 2} \propto \mathrm{C}\)

(c) \(\mathrm{t}_{1 / 2} \propto \mathrm{C}^0\)

(d) \(\mathrm{t}_{1 / 2} \propto \mathrm{C}^{\mathrm{U} / 2}\)

30. In the sequence of raction

\(k_3>k_2>k_1\), then the rate determining step of the raction is

(a) \(\mathrm{A} \rightarrow \mathrm{B}\)

(b) \(\mathrm{B} \rightarrow \mathrm{C}\)

(c) \(\mathrm{C} \rightarrow \mathrm{D}\)

(d) \(\mathrm{A} \Rightarrow \mathrm{D}\)

31. For a Zero order raction, the plot of conc. of products vs time is linear with

(a) +ve slope and zero intercept

(b) -ve slope and zero intercept

(c) +ve slope and non-zero intercept

(d) -ve slope and non-zero intercept

32. A first order reaction has a half-life period of then the rate constant will be

(a) \(10^{-4} \mathrm{Sec}^{-1}\)

(b) \(10^{-3} \mathrm{Sec}^{-1}\)

(c) \(10^{-1} \mathrm{Sec}^{-1}\)

(d) \(6.93 \times 10^{-3} \mathrm{Sec}^{-1}\)

33. Ethyl acetate is hydrolysed in acidic medium. Its order of reaction and molecularity are respectively

(a) 1 and 1

(b) 1 and 2

(c) 2 and 1

(d) 2 and 2

34. Which of the following is a first order reaction?

(a) \(2 \mathrm{H}_2 \mathrm{O}_{2(\text { (aq) }} \stackrel{\mathrm{x}}{\longrightarrow} 2 \mathrm{H}_2 \mathrm{O}+\mathrm{O}_{2(\mathrm{~g})}\)

(b) \(2 \mathrm{HI} \rightarrow \mathrm{H}_2+\mathrm{I}_2\)

(c) \(2 \mathrm{NO}_2 \rightarrow 2 \mathrm{NO}+\mathrm{O}_2\)

(d) \(2 \mathrm{NO}+\mathrm{O}_2 \rightarrow 2 \mathrm{NO}_2\)

35. If a is the initial concentration and \(K\) is the rate constant of a zero reaction, the time for the reaction to go to completion will be

(a) \(\frac{k}{a}\)

(b) \(\frac{\mathrm{a}}{\mathrm{k}}\)

(c) \(\frac{a}{2 k}\)

(d) \(\frac{k}{2 a}\)

36. The activation energy for the forward reaction \(\mathrm{X} \rightarrow \mathrm{Y}\) is \(80 \mathrm{k} . \mathrm{J}\). The heat of reaction is \(200 \mathrm{k.J}\). The activation energy for the reaction \(B \rightarrow A\) will be

(a) \(80 \mathrm{~kJ}\)

(b) \(120 \mathrm{~kJ}\)

(c) \(280 \mathrm{~kJ}\)

(d) \(200 \mathrm{~kJ}\)

37. For a first order reaction, the ratio of times to complete \(99.9 \%\) and half of the raction is

(a) 2

(b) 3.323

(c) 6.656

(d) 10

38. On addition of \(\mathrm{AgNO}_3\) to \(\mathrm{NaCL}\). White ppt occurs

(a) Instantaneously

(b) with a measurable speed

(c) slowly

(d) depending on condition

39. The hydrolysis of ethyl acetate was carried out separately with \(0.005 \mathrm{M} \mathrm{HC}\) and \(0.05 \mathrm{M} \mathrm{H}_2 \mathrm{SO}_4\). The rate constants were found to be \(K_1\) and \(K_2\) respectively. Then

(a) \(\mathrm{k}_1=\mathrm{k}_2\)

(b) \(\mathrm{k}_1>\mathrm{k}_2\)

(c) \(\mathrm{k}_1<\mathrm{k}_2\)

(d) \(k_2=2 k_1\)

40.

The above plot is for order reaction to calculate value of rate constant.

(a) Second

(b) First

(c) Zero

(d) First and Zero

41. The half-life period for a first order reaction is 69.3 S. Its rate constantis

(a) \(10^{-2} \mathrm{~S}^{-1}\)

(b) \(10^{-4} \mathrm{~S}^{-1}\)

(c) \(10 \mathrm{~S}^{-1}\)

(d) \(10^2 \mathrm{~S}^{-1}\)

42. For a first order reaction we have \(k=100\) \(\operatorname{Sec}^{-1}\). The time for completion of \(50 \%\) reaction is

(a) 1 millisec

(b) 4 millisec

(c) 7 millisec

(d) 10 millisec

43. What is the half life of a radioactive substance if \(75 \%\) of its given amount disintegrate in 60 min?

(a) \(30 \mathrm{~min}\)

(b) \(45 \mathrm{~min}\)

(c) \(75 \mathrm{~min}\)

(d) \(90 \mathrm{~min}\)

44. The influence of temperature on reaction rate is predicted by

(a) Kirchoff's equation

(b) Arrhenious equation

(c) Van der wall's equation

(d) Kinetic equation

45. For the reaction \(A \rightarrow B\) when concentration of \(A\) is made 1.5 times the rate of reaction becomes 1.837 times. The order of reaction is

(a) 1

(b) 1.5

(c) 2

(d) 2.5

46. What is the order of a reaction which has arate expression rate \(=\mathbf{k} \mid \mathbf{A}]^{\mathbf{s i 2}}\left[\left.\mathrm{B}\right|^{-19}\right.\) ?

(a) \(\frac{3}{2}\)

(b) \(\frac{1}{2}\)

(c) Zero

(d) 1

47. The minimum energy needed to convert a reactant into product is called

(a) Potential energy

(b) Kinetic energy

(c) Threshold energy

(d) Activation energy

48. Threshold enerlgy in a reaction is equal to

(a) activation energy

(b) activation energy - normal energy

(c) activation energy + normal energy

(d) normal enerlgy of reactants only

49. The rate of a chemical reaction depends on

(a) Atomic Mass

(b) Equivalent Mass

(c) Molecular Mass

(d) Active Mass

50. For a General Chemical change \(2 \mathrm{~A}+3 \mathrm{~B} \rightarrow\) products, the rates with respect to \(A\) is \(r_1\) and with respect to \(B\) is \(r_2\). The rates \(r_1\) and \(r_2\) are related as

(a) \(3 r_1=2 r_2\)

(b) \(r_1=r_2\)

(c) \(2 r_1=3 r_2\)

(d) \(r_1{ }^2=2 r_2\)