The thermodynamic efficiency of cell is given by

Reason : Neither oxidation nor reduction can take place alone.

${\mathrm{A}}_2+{\mathrm{B}}_2\to 2\mathrm{AB} ; \mathrm{R}.\mathrm{O}.\mathrm{R}.=\mathrm{k}{\left[{\mathrm{A}}_2\right]}^{\text{'}}{\left[{\mathrm{B}}_2\right]}^{\mathrm{b}}$

Order of reaction with respect to ${\mathrm{A}}_2$ and ${\mathrm{B}}_2$ are respectively:

For a reaction the initial rate is given as:${\mathrm{R}}_0=\mathrm{k}{\left[\mathrm{A}\right]}_0^2{\left[\mathrm{B}\right]}_0$ by what factor, the initial rate of reaction will increase if initial concentration of $\mathrm{A}$ is taken $1.5$ times and of $\mathrm{B}$ is tripled?

Which of the following expressions is correct for zero order and first order respectively [where a is initial concentration]?