Types of Elementary Reactions

Q. The time for half life period of a certain reaction, $A\to \text{Products}$ is 1 hour. When the initial concentration of the reactant 'A', is $2.0{\text{mol L}}^{-1}$, how much time (in hour) does it take for its concentration to come from $0.50{\text{mol L}}^{-1}$ to $0.25{\text{mol L}}^{-1}$, if it is a zero order reaction?

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

Q. Which of the following represents the rate law for the following reversible reaction?

1. $-\frac{d\left[A\right]}{dt}=k_1\left[A\right]+k_2\left[B\right]$
2. $\frac{+d\left[A\right]}{dt}=k_1\left[A\right]-k_2\left[B\right]$
3. $-\frac{d\left[B\right]}{dt}=k_1\left[A\right]-k_2\left[B\right]$
4. $-\frac{d\left[B\right]}{dt}=k_1\left[A\right]-k_2\left[B\right]$

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. 5.571 M

3. 55.71 M

4. 7.155 M

Q.

A substance undergoes first order decomposition involving two parallel first order reaction as :

The mol percent of B in the product is :

1. 76.83

2. 30.16

3. 69.84

4. 23.17

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