AIPMT 2007 | Chemical Kinetics Question 52 | Chemistry

AIPMT 2007

MCQ (Single Correct Answer)

-1

In a first-order reaction A $$ \to $$ B, if k is rate constant and initial concentration of the reactant A is 0.5 M, then the half-life is

$${{\log 2} \over k}$$

$${{\log 2} \over {k\sqrt {0.5} }}$$

$${{\ln 2} \over k}$$

$${{0.693} \over {0.5k}}$$

AIPMT 2007

MCQ (Single Correct Answer)

-1

If 60% of a first order reaction was completed in 60 minutes, 50% of the same reaction would be completed in approximately
(log 4 = 0.60, log 5 = 0.69)

45 minutes

60 minutes

40 minutes

50 minutes

AIPMT 2006

MCQ (Single Correct Answer)

-1

For the reaction, 2A + B $$ \to $$ 3C + D, which of the following does not express the reaction rate?

$$ - {{d\left[ A \right]} \over {2dt}}$$

$$ - {{d\left[ C \right]} \over {3dt}}$$

$$ - {{d\left[ B \right]} \over {dt}}$$

$$ {{d\left[ D \right]} \over {dt}}$$

AIPMT 2006

MCQ (Single Correct Answer)

-1

Consider the reaction : N_2(g) + 3H_2(g) $$ \to $$ 2NH_3(g)

The equality relationship between $${{d\left[ {N{H_3}} \right]} \over {dt}}$$ and $$ - {{d\left[ {{H_2}} \right]} \over {dt}}$$ is

$${{d\left[ {N{H_3}} \right]} \over {dt}} = - {{d\left[ {{H_2}} \right]} \over {dt}}$$

$${{d\left[ {N{H_3}} \right]} \over {dt}} = - {1 \over 3}{{d\left[ {{H_2}} \right]} \over {dt}}$$

$$ + {{d\left[ {N{H_3}} \right]} \over {dt}} = - {2 \over 3}{{d\left[ {{H_2}} \right]} \over {dt}}$$

$$ + {{d\left[ {N{H_3}} \right]} \over {dt}} = - {3 \over 2}{{d\left[ {{H_2}} \right]} \over {dt}}$$

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