(a) The reaction between A_2( g ) and B_2( g ) was carried out in a sealed isothermal container. The rate law for the reaction was found to be: Rate…

The reaction between $\displaystyle \mathrm{A}_{2}(\mathrm{~g})$ and $\displaystyle \mathrm{B}_{2}(\mathrm{~g})$ was carried out in a sealed isothermal container. The rate law for the reaction was found to be : \[\text { Rate }=\mathrm{k}\left[\mathrm{~A}_{2}\right]\left[\mathrm{B}_{2}\right] \] If $\displaystyle 1$ mole of $\displaystyle \mathrm{A}_{2}(\mathrm{~g})$ was added to the reaction chamber and the temperature was kept constant, then predict the change in rate of the reaction and the rate constant.

Reactant 'A' underwent a decomposition reaction. The concentration of 'A' was measured periodically and recorded in the table given below :

Time/Hours	[A]/M
$\displaystyle 0$	$\displaystyle 0.88$
$\displaystyle 1$	$\displaystyle 0.44$
$\displaystyle 2$	$\displaystyle 0 \cdot 22$
$\displaystyle 3$	$\displaystyle 0 \cdot 11$

Based on the above data, predict the order of the reaction and write the expression for the rate law.