320207 If decomposition of hydrogen peroxide is a first order reaction, it's rate law equation can be represented as

320208 The rate constant for the reaction,
$2{\mathrm{N}}_2{\mathrm{O}}_5⟶4{\mathrm{NO}}_2+{\mathrm{O}}_2\text{ is }3.0\times {10}^{-5}{\mathrm{s}}^{-1}\text{. }$
If the rate is $2.40\times {10}^{-5}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{S}}^{-1}$, then the concentration of ${\text{N}}_{\text{2}}{\text{O}}_{\text{5}}$ (in mol ${\text{L}}^{-1}$) is

320206 A reaction is first order with respective to $\mathrm{A}$ and second order with respective to $\mathrm{B}$. What is the effect on reaction rate if concentration of $\mathrm{B}$ is increase 3 times?

320207 If decomposition of hydrogen peroxide is a first order reaction, it's rate law equation can be represented as

320208 The rate constant for the reaction,
$2{\mathrm{N}}_2{\mathrm{O}}_5⟶4{\mathrm{NO}}_2+{\mathrm{O}}_2\text{ is }3.0\times {10}^{-5}{\mathrm{s}}^{-1}\text{. }$
If the rate is $2.40\times {10}^{-5}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{S}}^{-1}$, then the concentration of ${\text{N}}_{\text{2}}{\text{O}}_{\text{5}}$ (in mol ${\text{L}}^{-1}$) is

320206 A reaction is first order with respective to $\mathrm{A}$ and second order with respective to $\mathrm{B}$. What is the effect on reaction rate if concentration of $\mathrm{B}$ is increase 3 times?

320207 If decomposition of hydrogen peroxide is a first order reaction, it's rate law equation can be represented as

320208 The rate constant for the reaction,
$2{\mathrm{N}}_2{\mathrm{O}}_5⟶4{\mathrm{NO}}_2+{\mathrm{O}}_2\text{ is }3.0\times {10}^{-5}{\mathrm{s}}^{-1}\text{. }$
If the rate is $2.40\times {10}^{-5}\mathrm{mol}{\mathrm{L}}^{-1}{\mathrm{S}}^{-1}$, then the concentration of ${\text{N}}_{\text{2}}{\text{O}}_{\text{5}}$ (in mol ${\text{L}}^{-1}$) is