Chemical Kinetics

For a first order reaction, (A) $\rightarrow$ Products, the concentration of A changes from $0.1$ M to $0.025$ M in $40$ minutes. The rate of reaction when the concentration of A is $0.01$ M is

For the reaction, $2\text{N}_2\text{O}_{5(g)} \rightarrow 4\text{NO}_{2(g)} + \text{O}_{2(g)}$ in liquid bromine, the rate of formation of $\text{NO}_2$ is $0.08\ \text{mol dm}^{-3}\text{min}^{-1}$. What is the rate of…

Identify the order of reaction if rate of reaction is independent of the reactant concentration?

An increase in the concentration of the reactants of a reaction leads to a change in

Which of the following statements is NOT true about the decomposition of ammonia on platinum metal?

Which of the statement is correct regarding the half-life of a first-order reaction?

For an elementary reaction, $2A + B \rightarrow A_2B$, if $r = k[A]^2[B]$ If the volume of a vessel is quickly reduced to half of its original volume, then the rate of reaction will be

For the reaction $\text{C}_2\text{H}_5\text{Br}_{(l)} \rightarrow \text{C}_2\text{H}_{4(g)} + \text{HBr}$, $r = K(\text{C}_2\text{H}_5\text{Br})$ What is order and molecularity of the reaction respectively ?

What is the order of reaction for the following? $2\text{H}_2\text{O}_2(l) \rightarrow 2\text{H}_2\text{O}(l) + \text{O}_2(g)$

For first order reaction, the rate constant for the decomposition of $\text{N}_2\text{O}_5$ is $6 \times 10^{-4}$ s$^{-1}$. Calculate half life period for decomposition in terms seconds

The decomposition of $\text{N}_2\text{O}_{5(g)}$ occurs as: $2\ \text{N}_2\text{O}_{5(g)} \rightarrow 4\ \text{NO}_{2(g)} + \text{O}_{2(g)}$. If initial concentration of $\text{N}_2\text{O}_{5(g)}$ is $1.63 \times…

For the first order reaction, 80 % of the reactant decomposes in 60 minutes. Calculate the half life of the reaction.