The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3 \times 10^{-5} \, s^{-1}$. If the rate is $2.40 \times 10^{-5} \, mol \, L^{-1} \, s^{-1}$,then the concentration of $N_2O_5$ (in $mol \, L^{-1}$) is

For a particular reaction,the variation of the rate constant with temperature is given by $\ln k_t = \ln k_0 + \left( \frac{\ln (2.5)}{10} \right) \times t$ $(t \geqslant 0 \, ^{\circ}C)$. Here,$k_0$ is the rate constant at $0 \, ^{\circ}C$ and $k_t$ is the rate constant at $t \, ^{\circ}C$. The temperature coefficient of the reaction,assuming that the rate constant increases by the same factor for every $10 \, ^{\circ}C$ rise in temperature,is:

Which of the following is a unimolecular reaction?

For the reaction,$H_{2(g)} + Br_{2(g)} \longrightarrow 2 HBr_{(g)}$,$r = k[H_2][Br_2]^{\frac{1}{2}}$. What is the molecularity and order of reaction respectively?

What is the molecularity of a reaction? Explain its types with examples.

For the reaction $2A + B \rightarrow \text{product}$,the rate of the reaction is $15 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$ when $[A] = 0.3 \ mol \ dm^{-3}$ and $[B] = 0.05 \ mol \ dm^{-3}$. What is the value of the rate constant if the reaction is first order in both the reactants?