Types of Elementary Reactions

Q.

What is the unit of rate constant for a zero-order reaction?

Q.

A reversible reaction is in equilibrium. If a factor is changed which affects it,

then

1. Only the speed of that reaction increases which nullifies the factor

   causing increase of speed

2. No difference

3. The speed of forward and backward reaction increases

4. The speed of forward and backward reaction decreases

Q. 68. How equilibrium constant for a reversible reaction is equal to ratio of rate constant of forward reaction to that of backward reaction?

Q.

For a consecutive reaction $R_1\stackrel{k_1}{\to }{R}_2{R}_1\stackrel{k_2}{\to }{R}_3$ If initial concentration of $R_1$ is 100 M and $k_1:k_2=1:0.15$ the value of $[R_2{]}_{max}$ is $[Given:k_1=4.0\times {10}^{-2}mi{n}^{-1}]$

1. 71.55 M

2. 55.71 M

3. 7.155 M

4. 5.571 M

Q.

For the elementary reaction M ⟶ N, the rate of disappearance of M increases by a factor of 8 upon doubling the concentration of M. The order of the reaction with respect to M is

(IIT-JEE-Advanced 2014)

1. 4
2. 3
3. 2
4. 1

Q. Select the equation for [B] at any time t in the following reaction. Let the initial concentration of A be $\left[A_0\right]$ and B and C be 0.

1. $\left[B\right]=\left[B{]}_0\left(\frac{k_1\left[A\right]}{k_1+k_2}\right)\right(1-e^{-(k_1+k_2)t})$
2. $\left[B\right]=\frac{k_1\left[A\right]}{k_1+k_2}(1-e^{(k_1+k_2)t})$
3. $\left[B\right]=\frac{k_1[A{]}_0}{k_1+k_2}(1-e^{-(k_1+k_2)t})$
4. $\left[B\right]=\frac{k_1[A{]}_0}{k_1+k_2}(1-e^{(k_1+k_2)t})$

Q. $N_2{O}_5\left(g\right)\to 2N{O}_2\left(g\right)+\frac{1}{2}{O}_2\left(g\right)$

In the above first order reaction the initial concentration of $N_2{O}_5$ is 2.40 $\times {10}^{-2}mol{L}^{-1}$ at 318 K. The concentration of $N_2{O}_5$ after 1 hour was $1.60\times {10}^{-2}mol{L}^{-1}$ . The rate constant of the reaction at 318 k is $x\times {10}^{-3}mi{n}^{-1}$ The value of x (Nearest integer) is

$[Given:log3=0.447,log5=0.699]$




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Q.
Which of the following is a correct expression for the integrated rate law of first order reaction : $A\to \text{Products}$ ?
Here,
$a=[A{]}_0=\text{Initial concentration of the reactant A}$
$(a-x)=\left[A\right]=\text{Concentration of the reactant A at time t}$

1. $\left[A\right]=[A{]}_0-kt$
2. $\left[A\right]=[A{]}_0+kt$
3. $[A{]}_0=[A]e^{-kt}$
4. $\left[A\right]=[A{]}_0{e}^{-kt}$