1
MCQ (Single Correct Answer)

AIPMT 2006

For the reaction, 2A + B $$ \to $$ 3C + D, which of the following does not express the reaction rate?
A
$$ - {{d\left[ A \right]} \over {2dt}}$$
B
$$ - {{d\left[ C \right]} \over {3dt}}$$
C
$$ - {{d\left[ B \right]} \over {dt}}$$
D
$$ {{d\left[ D \right]} \over {dt}}$$

Explanation

Given,

2A + B $$ \to $$ 3C + D

Rate of reaction =

$$ - {1 \over 2}{{d\left[ A \right]} \over {dt}} = - {{d\left[ B \right]} \over {dt}}$$ = $${1 \over 3}{{d\left[ C \right]} \over {dt}} = {{d\left[ C \right]} \over {dt}}$$

2
MCQ (Single Correct Answer)

AIPMT 2006

Consider the reaction :  N2(g) + 3H2(g) $$ \to $$ 2NH3(g)

The equality relationship between $${{d\left[ {N{H_3}} \right]} \over {dt}}$$ and $$ - {{d\left[ {{H_2}} \right]} \over {dt}}$$ is
A
$${{d\left[ {N{H_3}} \right]} \over {dt}} = - {{d\left[ {{H_2}} \right]} \over {dt}}$$
B
$${{d\left[ {N{H_3}} \right]} \over {dt}} = - {1 \over 3}{{d\left[ {{H_2}} \right]} \over {dt}}$$
C
$$ + {{d\left[ {N{H_3}} \right]} \over {dt}} = - {2 \over 3}{{d\left[ {{H_2}} \right]} \over {dt}}$$
D
$$ + {{d\left[ {N{H_3}} \right]} \over {dt}} = - {3 \over 2}{{d\left[ {{H_2}} \right]} \over {dt}}$$

Explanation

N2(g) + 3H2(g) $$ \to $$ 2NH3(g)

Rate = $${{ - d\left[ {{N_2}} \right]} \over {dt}} = - {1 \over 3}{{d\left[ {{H_2}} \right]} \over {dt}} = {1 \over 2}{{d\left[ {N{H_3}} \right]} \over {dt}}$$

$$ \Rightarrow $$$${{d\left[ {N{H_3}} \right]} \over {dt}} = - {2 \over 3}{{d\left[ {{H_2}} \right]} \over {dt}}$$
3
MCQ (Single Correct Answer)

AIPMT 2005

For a first order reaction A $$ \to $$ B the reaction rate a reactant concentration of 0.01 M is found to be 2.0 $$ \times $$ 10$$-$$5 mol L$$-$$1 s$$-$$1. The half-life period of the reaction is
A
30 s
B
220 s
C
300 s
D
347 s

Explanation

Given [A] = 0.01 M

Rate = 2.0 × 10–5 mol L–1 S–1

For a first order reaction

Rate = k[A]

k = $${{2 \times {{10}^{ - 5}}} \over {0.01}} = 2 \times {10^{ - 3}}$$

$$ \Rightarrow $$ $${t_{1/2}} = {{0.693} \over {2 \times {{10}^{ - 3}}}} = 347\,\sec $$
4
MCQ (Single Correct Answer)

AIPMT 2005

The rate of reaction between two reactions A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is
A
2
B
$$-$$2
C
1
D
$$-$$1

Explanation

A + B $$ \to $$ Product

Rate $$ \propto $$ [A]x [B]y .......(1)

The rate of the reaction decreases by a factor of 4 if the concentration of reactant B is doubled.

$${r \over 4}$$ $$ \propto $$ [A]x [2B]y ......(2)

From equation (1) and (2), we get

$${\left( {{1 \over 2}} \right)^y} = 4$$

$$ \Rightarrow $$ y = -2

$$ \therefore $$ Order of this reaction with respect to reactant B is -2.

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