Molecularity of Reaction

1. Initial rate of reaction is $8\times {10}^{-9}{\text{mol L}}^{-1}{\text{S}}^{-1}$
2. When $A$ is reduced to $0.06mol{L}^{-1}$ then rate becomes $3.89\times {10}^{-9}mol{L}^{-1}Se{c}^{-1}$
3. When $A$ is reduced to $0.06mol{L}^{-1}$ then $B$ will be $0.16mol{L}^{-1}$
4. All are correct

1. $15.1kJmo{l}^{-1}$
2. $342kJmo{l}^{-1}$
3. $269kJmo{l}^{-1}$
4. $34.7kJmo{l}^{-1}$

Calculate the enthalpy change for the process

CCl_4(g) → C_(g) + 4Cl_(g)

and calculate bond enthalpy of C–Cl in CCl_4(g).

Δ_vapH^θ (CCl₄) = 30.5 kJ mol^–1.

Δ_fH^θ (CCl₄) = –135.5 kJ mol^–1.

Δ_aH^θ (C) = 715.0 kJ mol^–1, where Δ_aH^θ is enthalpy of atomisation

Δ_aH^θ (Cl₂) = 242 kJ mol^–1

Define stoichiometry.

The activation energy of a chemical reaction can be determined by

1. Evaluating rate constant at standard temperature

2. Changing concentration of reactants

3. Evaluating velocities of reaction at two different temperatures

4. Evaluating rate constants at two different temperatures

Inversion of cane sugar is a pseudo first-order reaction. Give reason.

The conversion of the molecule $\mathrm{X}\mathrm{To}\mathrm{Y}$follows second-order kinetics. If the concentration $\mathrm{X}$ is increased to three times, How will it affect the rate of formation of $\mathrm{Y}$?

1. If both statements are TRUE and statement -2 is the correct explanation of statement-1
2. If both the statements are TRUE but statement-2 is NOT the correct explanation of statement-1
3. If statement-1 is TRUE and statement-2 is FALSE
4. If statement-1 is FALSE and statement-2 is TRUE

1. $10\text{min};20\text{min}$
2. $2\times {10}^{-3}\text{min};4\times {10}^{-3}\text{min}$
   
3. $25\text{min};50\text{min}$
4. $250\text{min};500\text{min}$

Assertion (A) Order and molecularity are same.

Reason (R) Order is determined experimentally and molecularity is the sum of the stoichimetric coeffcient of rate determining elementary step.

(a) Both assertion and reason are correct and the reason is correct explanation of assertion
(b) Both assertion and reason are correct, but reason does not explain assertion.
(c) Assertion is correct, but reason is incorrect
(d) Both assertion and reason are incorrect
(e) Assertion is incorrect but reason is correct.

In what condition do order and molecularity of a reaction become equal?

1. $24.0min$
2. $27.3min$
3. $48.0min$
4. $49.4min$

Why can't molecularity of any reaction be equal to zero?

1. $k\left[A{]}^n\right[B{]}^n=-\frac{d\left[A\right]}{dt}=-\frac{d\left[B\right]}{dt}=+\frac{d\left[C\right]}{dt}$
2. $k\left[A{]}^n\right[B{]}^n=+\frac{d\left[A\right]}{dt}=+\frac{d\left[B\right]}{dt}=+\frac{d\left[C\right]}{dt}$
3. $k\left[A{]}^n\right[B{]}^n=-2\times \frac{d\left[A\right]}{dt}=-3\times \frac{d\left[B\right]}{dt}=+5\times \frac{d\left[C\right]}{dt}$
4. $k\left[A{]}^n\right[B{]}^n=\frac{-1}{2}\times \frac{d\left[A\right]}{dt}=\frac{-1}{3}\times \frac{d\left[B\right]}{dt}=\frac{+1}{5}\times \frac{d\left[C\right]}{dt}$

1. 2 M
2. 4 M
3. $6.67\times {10}^{-3}M$
4. 0.08 M

The order of the reaction is decided by

1. Pressure

2. Temperature

3. Molecularity

4. Mechanism of reaction as well as the relative concentration of reactants

1. $1.2\times {10}^{-4}mole{L}^{-1}mi{n}^{-1}and2.2\times {10}^{-4}mi{n}^{-1}$
2. $1.2\times {10}^{-4}mole{L}^{-1}mi{n}^{-1}and8.8\times {10}^{-4}mi{n}^{-1}$
3. $4.8\times {10}^{-4}mole{L}^{-1}mi{n}^{-1}and2.2\times {10}^{-4}mi{n}^{-1}$
4. $2.4\times {10}^{-4}mole{L}^{-1}mi{n}^{-1}and4.4\times {10}^{-4}mi{n}^{-1}$

1. $C{H}_{3}Cl>(C{H}_3{)}_{2}CHCl>C{H}_{3}C{H}_{2}Cl>(C{H}_3{)}_{3}CCl$
2. $C{H}_{3}Cl>C{H}_{3}C{H}_{2}Cl>(C{H}_3{)}_{2}CHCl>(C{H}_3{)}_{3}CCl$
3. $C{H}_{3}C{H}_{2}Cl>C{H}_{3}Cl>(C{H}_3{)}_{2}CHCl>(C{H}_3{)}_{3}CCl$
4. $(C{H}_3{)}_{2}CHCl>C{H}_{3}C{H}_{2}Cl>C{H}_{3}Cl>(C{H}_3{)}_{3}CCl$

In any unimolecular reaction ......... .
(a) only one reacting species is involved in the rate determining step
(b) the order and the molecularity of slowest step are equalto one
(c) the molecularity of the reaction is one and order is zero
(d) both molecularity and order of the reaction are one

1. It is experimentally determined
2. It is meant for the reaction and not for its individual steps
3. It may or may not be whole number.
4. It can never be zero

1. $3\times {10}^{-4}$
2. $2\times {10}^{-4}$
3. $\frac{4}{3}\times {10}^{-4}$
4. $4\times {10}^{-4}$

1. If both statements are TRUE and statement -2 is the correct explanation of statement-1
2. If both the statements are TRUE but statement-2 is NOT the correct explanation of statement-1
3. If statement-1 is TRUE and statement-2 is FALSE
4. If statement-1 is FALSE and statement-2 is TRUE

Why molecularity is applicable only for elementary reactions and order is applicable for elementary as well as complex reactions?

was found to be $3\times {10}^{-2}mol{L}^{-1}{s}^{-1}$
Then calculate the value of rate of disappearance of $N_2{O}_5$

1. $3\times {10}^{-2}mol{L}^{-1}{s}^{-1}$
2. $6\times {10}^{-2}mol{L}^{-1}{s}^{-1}$
3. $1.5\times {10}^{-2}mol{L}^{-1}{s}^{-1}$
4. $1.2\times {10}^{-1}mol{L}^{-1}{s}^{-1}$

1. Reversible step
2. From overall reaction
3. Fastest step
4. Slowest step

In a reaction between A and B, the initial rate of reaction (r₀) was measured for different initial concentrations of A and B as given below:

A/ mol L−1	0.20	0.20	0.40
B/ mol L−1	0.30	0.10	0.05
r0/ mol L−1 s−1	5.07 × 10−5	5.07 × 10−5	1.43 × 10−4

What is the order of the reaction with respect to A and B?