A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will

In a gaseous reaction 

${A_{2\left( g \right)}} \longrightarrow {B_{\left( g \right)}} + \frac{1}{2}\,{C_{\left( g \right)}}$ the increase in pressure from $100\, mm$ to $120\, mm$ is noticed in $5\,\min$. The rate of dissappearence of $A_2$ in $mm\, min^{-1}$ is

The rate constant for the reaction $2N_2O_5 \to  4NO_2 + O_2$ is $3.0\times10^{-5}\, sec^{-1}$. If rate is $2.40\times10^{-5}\, M\, sec^{-1}$, then the concentration of $N_2O_5$ (in $M$) is ?

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 $?$

Order of radioactive disintegration reaction is

The rates of a certain reaction $(dc/dt)$ at different times are as follows

Time                                 Rate (mole $litre^{-1}\,sec^{ -1}$ )

$0$                                        $2.8 \times {10^{ - 2}}$

$10$                                      $2.78 \times {10^{ - 2}}$

$20 $                                     $2.81 \times {10^{ - 2}}$

$30$                                       $2.79 \times {10^{ - 2}}$

The reaction is