For a reaction, $I^-+OCl^-  \to IO^-+Cl^-$ in a aqueous medium, the rate of reaction is given by $\frac{{d[{IO^ - }]}}{{dt}} = k[{I^ - }][OC{l^ - }]$ The overall order of reaction is

For the following reaction: $NO_2(g) + CO(g) \to NO(g) + CO_2(g)$, the rate law is: Rate $= k \,[NO_2]^2$. If $0.1\,mole$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?

The rate law for the reaction below is given by the expression $k\left[ A \right]\left[ B \right]$ 

                                          $A + B \to$ Product 

If the concentration of $B$ is increased from $0.1$ to $0.3\, mole$, keeping the value of $A$ at $0.1\, mole$, the rate constant will be

In the reaction : $P + Q \longrightarrow  R + S$ the time taken for $75\%$ reaction of $P$ is twice the time taken for $50\%$ reaction of $P$. The concentration of $Q$ varies with reaction time as shown in the figure. The overall order of the reaction is

units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.

$(iv)$ $C _{2} H _{5} Cl ( g ) \rightarrow C _{2} H _{4}( g )+ HCl ( g ) \quad$ Rate $=k\left[ C _{2} H _{5} Cl \right]$