NEET Definition, Rate Constant, Rate Law Practice Questions With Solutions

NEET Chemistry Definition, Rate Constant, Rate Law Practice Questions

Question 1.

Which of the following expression is correct for the reaction given below? \(2 \mathrm{HI}_{(g)} \rightarrow \mathrm{H}_{2(g)}+\mathrm{I}_{2(g)}\)

A\(\dfrac{-\Delta[\mathrm{H}I]}{\Delta t}=\dfrac{2 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\)

B\(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4\Delta\left[\mathrm{I}_2\right]}{\Delta t}\)

C\(\dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{4 \Delta\left[\mathrm{H}_2\right]}{\Delta t}\)

D\( \dfrac{-\Delta[\mathrm{HI}]}{\Delta t}=\dfrac{\Delta\left[\mathrm{H}_2\right]}{\Delta t}\)

Question 2.

For a reaction \(3A \rightarrow 2B\)
The average rate of appearance of B is given by \(\Delta [B] \over \Delta t\) .
The correct relation between the average rate of appearance of B with the average rate of disappearance of A is:

A\(-\Delta [A] \over \Delta t\)

B\(-3\Delta [A] \over 2\Delta t\)

C\(-2\Delta [A] \over 3\Delta t\)

D\(\Delta [A] \over \Delta t\)

Question 3.

For a chemical reaction, 4A + 3B → 6C + 9D
rate of formation of C is 6 × 10 ^–2 mol L ^–1 s ^–1 and rate of disappearance of A is 4 × 10 ^–2 mol L ^–1 s ^–1 . The rate of reaction and amount of B consumed in interval of 10 seconds , respectively will be:

A1 × 10^–2 mol L^–1 s^–1 and 30 × 10^–2 mol L^–1

B10 × 10^–2 mol L^–1 s^–1 and 10 × 10^–2 mol L^–1

C1 × 10^–2 mol L^–1 s^–1 and 10 × 10^–2 mol L^–1

D10 × 10^–2 mol L^–1 s^–1 and 30 × 10^–2 mol L^–1

Question 4.

For the reaction, 2A → B, rates= k[A]². If the concentration of reactant is doubled, then the:

Arate of reaction will be doubled.

Brate constant will remain unchanged, however rate of reaction is directly proportional to the rate constant.

Crate constant will change since the rate of reaction and rate constant are directly proportional to each other.

Drate of reaction will increase by four times.

Question 5.

For the chemical reaction

N_{2} (g) + 3 H_{2} (g)

⇌

2 {NH}_{3} (g)

the correct option is:

3 \frac{d [H_{2}]}{dt} = 2 \frac{d [{NH}_{3}]}{dt}

- \frac{1}{3} \frac{d [H_{2}]}{dt} = - \frac{1}{2} \frac{d [{NH}_{3}]}{dt}

- \frac{d [N_{2}]}{dt} = 2 \frac{d [{NH}_{3}]}{dt}

- \frac{d [N_{2}]}{dt} = \frac{1}{2} \frac{d [{NH}_{3}]}{dt}

Question 6.

The correct statement among the following is:

Athe rate of a first-order reaction does not depend on reactant concentration; the rate of a second-order reaction does depend on reactant concentrations.

Bthe half-life of a first-order reaction does not depend on [A]_o; the half-life of a second-order reaction does depend on [A]₀

Ca first-order reaction can be catalyzed; a second-order reaction cannot be catalyzed.

Dthe rate of a first-order reaction does depend on reactant concentrations; the rate of a second-order reaction does not depend on reactant concentrations

Question 7.

Which quantity is altered when a catalyst is introduced during a chemical reaction?

1.	Internal energy	2.	Enthalpy
3.	Activation energy	4.	Entropy

AInternal energy

BEnthalpy

CActivation energy

DEntropy

Question 8.

In a reaction, A + B → Product, the rate is doubled when the concentration of B is doubled, and the rate increases by a factor of 8, when the concentrations of both the reactants (A and B) are doubled. The rate law for the reaction can be written as:

ARate = k[A][B]²

BRate = k[A]²[B]²

CRate = k[A][B]

DRate = k[A]²[B]

Question 9.

The unit of rate constant for a zero-order reaction is:

s^{- 1}

mol

L^{- 1} s^{- 1}

L

{mol}^{- 1} s^{- 1}

L^{2} {mol}^{- 2} s^{- 1}

Question 10.

Which of the following statements about the order of reaction is incorrect?

AOrder is not influenced by the stoichiometric coefficient of the reactants.

BOrder of reaction is the sum of power to the concentration terms of reactants to express the rate of reaction.

CThe order of reaction is always a whole number.

DOrder can be determined by experiments only.

Question 1.

For the reaction, \(\mathrm{N}_2+3 \mathrm{H}_2 \rightarrow 2 \mathrm{NH}_3,\) if, \(\dfrac{d[NH_{3}]}{dt} \ = \ 2\times 10^{-4} \ mol \ L^{-1} \ s^{-1}\), the value of \(\dfrac{-d[H_{2}]}{dt}\) would be:

A\(3 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)

B\(4 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)

C\(6 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1} \)

D\(1 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\)

Question 2.

For the reaction, A + B → products, it is observed that-
(1) On doubling the initial concentration of A only, the rate of reaction is also doubled and
(2) On doubling the initial concentrations of both A and B, there is a change by a factor of 8 in the rate of the reaction.
The rate of this reaction is given by:

r a t e = k

[A]^{2} [B]

r a t e = k

[A] [B]^{2}

r a t e = k

[A]^{2} [B]^{2}

r a t e = k

[A] [B]

Question 3.

In the reaction,

{BrO}_{3}^{-} (aq) + 5 {Br}^{-} (aq) + 6 H^{+} \to

3Br₂(l)+3H₂O(l)
The rate of appearance of bromine (Br₂) is related to the rate of disappearance of bromide ions:

\frac{d [B r_{2}]}{d t} = - \frac{3}{5} \frac{d [B r^{-}]}{d t}

\frac{d [B r_{2}]}{d t} = - \frac{5}{3} \frac{d [B r]}{d t}

\frac{d [B r_{2}]}{d t} = \frac{5}{3} \frac{d [B r^{-}]}{d t}

\frac{d [B r_{2}]}{d t} = \frac{3}{5} \frac{d [B r^{-}]}{d t}

Question 4.

The half-life period of a first-order reaction is 1386 s. The specific rate constant of the reaction is:

5.0 \times 10^{- 3} s^{- 1}

0.5 \times 10^{- 2} s^{- 1}

0.5 \times 10^{- 3} s^{- 1}

5.0 \times 10^{- 2} s^{- 1}

Question 5.

In the reaction, 3 A \to 2 B the

rate of reaction

\frac{+ d [B]}{dt}

is equal to:-

- \frac{3}{2} \frac{d [A]}{dt}

- \frac{2}{3} \frac{d [A]}{dt}

- \frac{1}{3} \frac{d [A]}{dt}

+ 2 \frac{d [A]}{dt}

Question 6.

If at a given instant, for the reaction 2N₂O₅→ 4NO₂ + O₂ rate and rate constant are 1.02 × 10^-4 and 3.4 × 10^-5 sec ^-1 respectively, then the concentration of

N_{2} O_{5}

at that time will be:

A1.732

m o l L -1

B3.0

m o l L -1

1.02

\times

10^{- 4}

m o l L -1

3.4

\times

10^{5}

m o l L -1

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NEET Definition, Rate Constant, Rate Law Practice Questions With Solutions

NEET Chemistry Definition, Rate Constant, Rate Law Practice Questions

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

Question 7.

Question 8.

Question 9.

Question 10.

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

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