Consider the following reaction in a batch reactor at constant volume:$()+2()2()+2()($a$)$ If hydrogen is in excess, how does the formation rate of nitrogen and water relateto the reaction rate of nitric oxide?$[3]($b$)$ Determine the composition of the reactor if the fractional conversion is $0\mathrm{.}8$ and theinitial composition was $10$ mol L$-1$ NO and $20$ mol L$-1$ H$2[5]($c$)$ If the reaction is first order in NO and second order in H$2.$ Write the rate law forthe reaction and find the units for the rate constant if the reaction progress ismeasured in concentration $($mol L$-1).[3]($d$)$ If the reaction progress is measured in partial pressure $($Pa$),$ write the rate law andfind the units for the rate constant.$[3]4.$A reversible reaction between hydrogen and iodine occurs as follows:H$2($g$)+$ I$2($g$)2$HI$($g$)$ Kc $=49\mathrm{.}0$ at $700$ KWhere Kc is the equilibrium constant.$($a$)$ If a $10$ L reaction vessel is fed with $1$ mole of H$2$ and $1$ mole I$2$ at $700$ K$,$ what arethe equilibrium concentrations of all components?$[8]($b$)$ If kr $=1\mathrm{.}20\backslash$times $10-3$ M$-1$s$-1$ at $700$ K$,$ what is the value of kf at the same temperature?Where kf is the forward reaction rate constant and kr is the reverse rate constant.$[2]($c$)$ If the forward reaction is endothermic, explain with justification how an increasein temperature affects the values of Kc$,$ kf and kr$?$