The rate law for the reaction R C l + N a O H ( a q ) → R O H + N a C l is given by Rate = k [ R C l ] . The rate of the reaction will be

Halved on reducing the concentration of alkyl halide to one half

Decreased on increasing the temperature of the reaction

Doubled on doubling the concentration of sodium hydroxide

Unaffected by increasing the temperature of the reaction

The rate law for the reaction R C l + N a O H ( a q ) → R O H + N a C l is given by Rate = k [ R C l ] . The rate of the reaction will be

Halved on reducing the concentration of alkyl halide to one half

N O 2 required for a reaction is produced by the decomposition of N 2 O 5 in C C l 4 as per the equation, 2 N 2 O 5 g → 4 N O 2 g + O 2 g . The initial concentration of N 2 O 5 is 3.00 m o l L - 1 and it is 2.75 m o l L - 1 after 30 minutes. The rate of formation of N O 2 is:

1.667 × 10 - 2 m o l L - 1 m i n - 1

8.333 × 10 - 3 m o l L - 1 m i n - 1

4.167 × 10 - 3 m o l L - 1 m i n - 1

2.083 × 10 - 3 m o l L - 1 m i n - 1

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The rate law for the reaction $R C l + N a O H (a q) \to R O H + N a C l$ is given by
Rate $= k [R C l]$ . The rate of the reaction will be

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Important Questions on Chemical Kinetics

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For an elementary chemical reaction, $A_{2} ⇄_{k_{- 1}}^{k_{1}} 2 A$ , the expression for $\frac{d [A]}{dt}$ is:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

In the following reaction; $x A \to y B$

$\log_{10} [- \frac{d [A]}{d t}] = \log_{10} [- \frac{d [B]}{d t}] + 0.3010$

‘A’ and ‘B’ respectively can be:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For the reaction

2 H_{2} (g) + 2 N O (g) \to N_{2} (g) + 2 H_{2} O (g)

the observed rate expression is, rate

= k_{f} {[NO]}^{2} [H_{2}]

. The rate expression for the reverse reaction is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

Consider the following reactions
$A \to P 1; B \to P 2; C \to P 3; D \to P 4$
The order of the above reactions are $a, b, c and d,$ respectively. The following graph is obtained when log[rate] vs.log[conc.] are plotted:

Question Image
Among the following, the correct sequence for the order of the reactions is :

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

A + 2 B \to C

, the rate equation for the reaction is given as

Rate

= k [A] [B]

If the concentration of A is kept the same but that of B is doubled what will happen to the rate itself?

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

The results given in the below table were obtained during kinetic studies of the following reaction: $2 A + B \to C + D$

Experiment	$[A] / {molL}^{- 1}$	$[B] / {molL}^{- 1}$	Initial rate/ ${molL}^{- 1} \min^{- 1}$
I	$0.1$	$0.1$	$6.00 \times 10^{- 3}$
II	$0.1$	$0.2$	$2.40 \times 10^{- 2}$
III	$0.2$	$0.1$	$1.20 \times 10^{- 2}$
IV	X	$0.2$	$7.20 \times 10^{- 2}$
V	$0.3$	Y	$2.88 \times 10^{- 1}$

X and Y in the given table are respectively :

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For a chemical reaction rate law is, rate

= K {[A]}^{2} [B] .

If [A] is doubled at constant

[B],

the rate of reaction.

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For a first order reaction

(A ⟶ P)

the rate constant is

5 \times 10^{- 3} \min^{- 1}

when the initial concentration of

A = 2 \times 10^{- 2} M

. If the initial concentration of

A

is doubled, what will be the rate constant (in

\min^{- 1}

) at the same temperature?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

The rate law for the reaction below is given by the expression

k [A] [B]

A + B \to P r o d u c t

If the concentration of

B

is increased from

0.1 to 0.3 mol

, keeping the value of

A

0.1 mol

, the rate constant will be:

HARD

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below:

O_{3} (g) + {Cl}^{•} \to O_{2} (g) + {ClO}^{•} (g)

...(i)

k_{i} = 5.2 \times 10^{9} L m o l^{- 1} s^{- 1}

{ClO}^{•} (g) + O^{•} (g) \to O_{2} (g) + {Cl}^{•} (g)

...(ii)

k_{i i} = 2.6 \times 10^{10} L m o l^{- 1} s^{- 1}

The closest rate constant for the overall reaction

O_{3} (g) + O^{•} (g) \to 2 O_{2} (g)

is:

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

Which of the following expression is correct for the rate of reaction given below ?

$5 {Br}^{-} (aq) + {BrO}_{3}^{-} (aq) + 6 H^{+} (aq) ⟶ 3 {Br}_{2} (aq) + 3 H_{2} O (l)$

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

Find the unit of the rate constant of a reaction represented with a rate equation, rate

= k {[A]}^{\frac{1}{2}} {[B]}^{\frac{3}{2}}

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

The rate constant for a second order reaction,

A \to

Product, is

1.62 M^{- 1} s^{- 1}

. What will be the rate of reaction when concentration of reactant is

2 \times 10^{- 3} M

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

For the following reactions

Question Image

where,

k_{s}

and

k_{e}

, are respectively, the rate constants for substitution and elimination, and

μ = \frac{k_{s}}{k_{e}}

, the correct option is ________

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

Which one of the following statements is not correct?

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

27 ° C

temperature, time required for

75 %

completion of a first order reaction is

20

seconds. What will be its rate constant?

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

The unit of second order reaction rate constant is;

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

N O_{2}

required for a reaction is produced by the decomposition of

N_{2} O_{5}

C C l_{4}

as per the equation,

2 N_{2} O_{5} (g) \to 4 N O_{2} (g) + O_{2} (g) .

The initial concentration of

N_{2} O_{5}

3.00 m o l L^{- 1}

and it is

2.75 m o l L^{- 1}

after 30 minutes. The rate of formation of

N O_{2}

is:

MEDIUM

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

Mechanism of a hypothetical reaction

X_{2} + Y_{2} \to 2 XY

is given below:

(i)

X_{2} \to X + X (fast)

(ii)

X + Y_{2} ⇌ XY + Y (slow)

(iii)

X + Y \to XY (fast)

The overall order of the reaction will be

EASY

Chemistry>Physical Chemistry>Chemical Kinetics>The Rate Law and Rate Constant

Decomposition of

X

exhibits a rate constant of

0 .05 μg / year

. How many years are required for the decomposition of

5 μg

X

into

2 .5 μg

The rate law for the reaction RCl+NaOH(aq)→ROH+NaCl is given by Rate =k[RCl] . The rate of the reaction will be

Important Questions on Chemical Kinetics

Learn and Prepare for any exam you want !

The rate law for the reaction $R C l + N a O H (a q) \to R O H + N a C l$ is given by
Rate $= k [R C l]$ . The rate of the reaction will be