Zero Order Reaction

Q. A first order reaction is 60% complete in 20 minutes. How long will the reaction take to be 84% complete?

1. 54 mins
2. 68 mins
3. 40 mins
4. 76 mins

Q. For reaction $A\to B$, rate constant of reaction at ${27}^{\circ }C$ is $1.2\times {10}^{-3}$ $M{s}^{-1}$. The only correct graph for the reaction is,

1. 
2. 
3. 
4. 

Q. The rate constant of the reaction $A\to B$ is $0.6\times {10}^{-3}\text{M/s}$. If the concentration of $A$ is $5\text{M}$, then concentration of $B$ after 20 minutes is :-

1. $3.60\text{M}$
2. $0.72\text{M}$
3. $1.08\text{M}$
4. $0.36\text{M}$

Q. The initial rate of zero order reaction of the gaseous reaction A(g) $\to$ 2B(g) is ${10}^{-2}$ M/min. If the initial concentration of A is 0.1 M, what would be the concentration of B after 60 sec?

1. 0.09 M
2. 0.01 M
3. 0.02 M
4. 0.002 M

Q. The following results have been obtained during the kinetic study of the reaction
$A+B⟶C+D$
$\begin{array}{cccc}\text{Experiment}& \text{[A]}& \text{[B]}& \text{Initial rate of}\\ & & & \text{formation of}\\ & & & \left(Mse{c}^{-1}\right)\\ \text{I}& 0.1& 0.1& 6.0\times {10}^{-3}\\ \text{II}& 0.3& 0.2& 7.2\times {10}^{-2}\\ \text{III}& 0.3& 0.4& 2.88\times {10}^{-1}\\ \text{IV}& 0.4& 0.1& 2.40\times {10}^{-2}\end{array}$
Determine the rate law of the above reaction.

1. Rate law $=k\left[A{]}^2\right[B]$
2. Rate law $=k\left[A\right]\left[B\right]$
3. Rate law $=k\left[A{]}^2\right[B{]}^2$
4. Rate law $=k\left[A\right][B{]}^2$

Q. Sita has to select one reaction out of zero order, first order, second order, and a third order reaction such that, the rate of reaction is constant throughout the reaction. Which one should she select?

1. Zero order reaction
2. First order reaction
3. Second order reaction
4. Third order reaction

Q. If the rate of a reaction is equal to the rate constant, the order of the reaction is:

1. 2
2. 3
3. \N
4. 1

Q. The units of rate constant and rate of reaction are identical for

1. zero order reaction
2. first order reaction
3. second order reaction
4. pseudo first order reaction

Q. The time required for $100\%$ completion of a zero order reaction is .
(a is the initial concentration and k is the rate constant)

1. $\frac{a}{k}$
2. $\frac{2k}{a}$
3. $ak$

Q. Sita has to select one reaction out of zero order, first order, second order, and a third order reaction such that, the rate of reaction is constant throughout the reaction. Which one should she select?

1. Zero order reaction
2. First order reaction
3. Second order reaction
4. Third order reaction

Q.

The rate constant of the reaction $A\to B$ is $0.6\times {10}^{-3}$ mole per second. If the concentration of B after 20 min is:

1. 1.08 M

2. 3.60 M

3. 0.36 M

4. 0.72 M

Q. The decomposition of dimethyl ether is a fractional order reaction. The rate of reaction is given by
$Rate=k(P_{C{H}_{3}OC{H}_3}{)}^{3/2}$. If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constant respectively?

1. $ba{r}^{\frac{-1}{2}}mi{n}^{-1},ba{r}^{2}mi{n}^{-1}$
2. $barmi{n}^{-1},ba{r}^{\frac{-1}{2}}mi{n}^{-1}$
3. $barmi{n}^{-1},ba{r}^{\frac{1}{2}}mi{n}^{-1}$
4. $barmi{n}^{-1},ba{r}^{2}mi{n}^{-1}$

Q. The decomposition of dimethyl ether is a fractional order reaction. The rate of reaction is given by
$Rate=k(P_{C{H}_{3}OC{H}_3}{)}^{3/2}$. If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constant respectively?

1. $barmi{n}^{-1},ba{r}^{\frac{1}{2}}mi{n}^{-1}$
2. $barmi{n}^{-1},ba{r}^{\frac{-1}{2}}mi{n}^{-1}$
3. $barmi{n}^{-1},ba{r}^{2}mi{n}^{-1}$
4. $ba{r}^{\frac{-1}{2}}mi{n}^{-1},ba{r}^{2}mi{n}^{-1}$

Q. Consider the zero order reaction
$R\to P$
Starting with 4 moles of R in a one litre container, after half an hour only 1 mole of R is left unreacted. The value of k for the reaction is:

1. $0.1mol{L}^{-1}mi{n}^{-1}$
2. $0.3mol{L}^{-1}mi{n}^{-1}$
3. $1mol{L}^{-1}mi{n}^{-1}$
4. $0.4mol{L}^{-1}mi{n}^{-1}$

Q. A first order reaction is 60% complete in 20 minutes. How long will the reaction take to be 84% complete?

1. 76 mins
2. 54 mins
3. 68 mins
4. 40 mins