Chemical Kinetics

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Chemical Kinetics - 05

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Q1. For the reaction H2(g) + Br2 (g) → 2HBr (g), the experimental data suggest, rate = k[H2][Br2]^1/2. The molecularity and order of the reaction are respectively *

1 point

2 and 1

2 and 1/2

2 and 3/2

1 and 2

Q2. The plot that represents the zero order reaction is *

1 point

Q3. The plot of concentration of the reactant vs time for are action is a straight line with a negative slope. The reaction follows a rate equation *

1 point

Second order

Zero order

Third order

First order

Q4. Rate = k[N2O]^0 = k. If the initial concentration of ther eactant is a mol Lit–1, the half-life period of the reaction is *

1 point

t1/2 = k/a

t1/2 = ak

t1/2 = 0

t1/2 = a/2k

Q5. Half life of a first order reaction is 4s and the initial concentration of the reactant is 0.12 M. The concentration of the reactant left after 16 s is *

1 point

0.015 M

0.06 M

0.03 M

0.0075 M

Q6. The reaction o BA follows first order kinetics. The time taken for 0.8 mole of A to produce 0.6 mole of B is 1 hour. What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of B? *

1 point

2 hr

1 hr

2.5 hr

1.5 hr

Q7. The rate of a first order reaction is 1.5 × 10–2 mol L–1 min–1 at 0.5 M concentration of the reactant. The half life of the reaction is *

1 point

0.383 min

7.53 min

23.1 min

8.73 min

Q8. The rate constant for a first order reaction whose half-life, is 480 seconds is *

1 point

2.88 × 10^–3 sec–1

1.44 sec–1

1.44 × 10^–3 sec–1

2.72 × 10^–3 sec–1

Q9. The rate constant of a first order reaction is 6.9 x 10-3 s-1. How much time will it take to reduce the initial concentration to its 1/8th value? *

1 point

300 sec

400 sec

200 sec

100 sec

Q10. A reaction proceeds by first order, 75% of this reaction was completed in 32 min. The time required for 50% completion is *

1 point

16 min

8 min

24 min

22 min

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