For a reaction,$2 \ N_2O_{5(g)} \longrightarrow 4 \ NO_{2(g)} + O_{2(g)}$. The $N_2O_5$ disappears at a rate of $0.06 \ mol \ dm^{-3} \ s^{-1}$. What is the rate of $NO_{2(g)}$ formation (in $mol \ dm^{-3} \ s^{-1}$)?

In the following reaction,$2H_2O_2 \to 2H_2O + O_2$,the rate of formation of $O_2$ is $36 \ g \ min^{-1}$. What is the rate of disappearance of $H_2O_2$ in $mol \ min^{-1}$?

Calculate the instantaneous rate $(r_{inst})$ based on the example problem $-1$ graphically for the times $250\ s$,$350\ s$,$450\ s$,and $600\ s$.

Consider the following reactant samples:
$I$. $1 \ mol$ of $A$ and $2 \ mol$ of $B$ in a $1 \ L$ vessel
$II$. $2 \ mol$ of $A$ and $2 \ mol$ of $B$ in a $2 \ L$ vessel
$III$. $0.2 \ mol$ of $A$ and $0.2 \ mol$ of $B$ in a $0.1 \ L$ vessel
Which reactant sample reacts at the highest rate if the reactants are in the gaseous state and do not follow a zero-order reaction?

What is the average rate of reaction when the change in concentration of product is $0.05 \ M$ in $20 \ s$ (in $M \ s^{-1}$)?

If the first order reaction involves gaseous reactants and gaseous products,the units of its rate are: