Chemical Kinetics

For the reaction $R \rightarrow P$, the concentration of a reactant changes from 0.03M to 0.02M in 25 minutes. Calculate the average rate of reaction using units of time both in minutes and seconds.

In a reaction, $2A \rightarrow Products$, the concentration of $A$ decreases from 0.5 mol L$^{-1}$ to 0.4 mol L$^{-1}$ in 10 minutes. Calculate the rate during this interval?

For a reaction, $A + B \rightarrow Product$; the rate law is given by, $r = k [A]^{1/2} [B]^2$. What is the order of the reaction?

The conversion of molecules $X$ to $Y$ follows second order kinetics. If concentration of $X$ is increased to three times how will it affect the rate of formation of $Y$?

A first order reaction has a rate constant $1.15 \times 10^{-3} \text{ s}^{-1}$. How long will 5 g of this reactant take to reduce to 3 g?

Time required to decompose $\text{SO}_2\text{Cl}_2$ to half of its initial amount is 60 minutes. If the decomposition is a first order reaction, calculate the rate constant of the reaction.

What will be the effect of temperature on rate constant?

The rate of the chemical reaction doubles for an increase of 10K in absolute temperature from 298K. Calculate $E_a$.

The activation energy for the reaction $2 \text{HI(g)} \rightarrow \text{H}_2 + \text{I}_2 (\text{g})$ is 209.5 kJ mol$^{-1}$ at 581K. Calculate the fraction of molecules of reactants having energy equal to or greater than activation energy?

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants. (i) $3\text{NO}(g) \rightarrow \text{N}_2\text{O}(g)$ Rate $= k[\text{NO}]^2$ (ii) $\text{H}_2\text{O}_2(\text{aq}) + 3\text{I}^-(\text{aq}) + 2\text{H}^+ \rightarrow 2\text{H}_2\text{O}(\text{l}) + \text{I}_3^-$ Rate $= k[\text{H}_2\text{O}_2][\text{I}^-]$ (iii) $\text{CH}_3\text{CHO}(\text{g}) \rightarrow \text{CH}_4(\text{g}) + \text{CO}(\text{g})$ Rate $= k[\text{CH}_3\text{CHO}]^{3/2}$ (iv) $\text{C}_2\text{H}_5\text{Cl}(\text{g}) \rightarrow \text{C}_2\text{H}_4(\text{g}) + \text{HCl}(\text{g})$ Rate $= k[\text{C}_2\text{H}_5\text{Cl}]$

For the reaction: $2\text{A} + \text{B} \rightarrow \text{A}_2\text{B}$, the rate $= k[\text{A}][\text{B}]^2$ with $k = 2.0 \times 10^{-6} \text{ mol}^{-2} \text{ L}^{2} \text{ s}^{-1}$. Calculate the initial rate of the reaction when $[\text{A}] = 0.1 \text{ mol L}^{-1}$, $[\text{B}] = 0.2 \text{ mol L}^{-1}$. Calculate the rate of reaction after $[\text{A}]$ is reduced to $0.06 \text{ mol L}^{-1}$.

The decomposition of $\text{NH}_3$ on platinum surface is zero order reaction. What are the rates of production of $\text{N}_2$ and $\text{H}_2$ if $k = 2.5 \times 10^{-4} \text{ mol}^{-1} \text{ L s}^{-1}$?

The decomposition of dimethyl ether leads to the formation of $\text{CH}_4$, $\text{H}_2$ and $\text{CO}$ and the reaction rate is given by Rate $= k[\text{CH}_3\text{OCH}_3]^{3/2}$. The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e., Rate $= k\left(p_{\text{CH}_3\text{OCH}_3}\right)^{3/2}$. If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?

Mention the factors that affect the rate of a chemical reaction.

A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is (i) doubled (ii) reduced to half?

What is the effect of temperature on the rate constant of a reaction? How can this effect of temperature on rate constant be represented quantitatively?

In a pseudo first order reaction in water, the following results were obtained: t/s: 0, 30, 60, 90 [A]/mol L$^{-1}$: 0.55, 0.31, 0.17, 0.085 Calculate the average rate of reaction between the time interval 30 to 60 seconds.

A reaction is first order in A and second order in B. (i) Write the differential rate equation. (ii) How is the rate affected on increasing the concentration of B three times? (iii) How is the rate affected when the concentrations of both A and B are doubled?

In a reaction between A and B, the initial rate of reaction ($r_0$) 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 $r_0$/mol L$^{-1}$s$^{-1}$: $5.07 \times 10^{-5}$, $5.07 \times 10^{-5}$, $1.43 \times 10^{-4}$ What is the order of the reaction with respect to A and B?

The following results have been obtained during the kinetic studies of the reaction:

Experiment | [A]/mol L$^{-1}$ | [B]/mol L$^{-1}$ | Initial rate of formation of D/mol L$^{-1}$ min$^{-1}$ I | 0.1 | 0.1 | $6.0 \times 10^{-3}$ II | 0.3 | 0.2 | $7.2 \times 10^{-2}$ III | 0.3 | 0.4 | $2.88 \times 10^{-1}$ IV | 0.4 | 0.1 | $2.40 \times 10^{-2}$ Determine the rate law and the rate constant for the reaction.