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$,$ calculate theequilibrium concentrations of all components?$($b$)$ If kr $=1\mathrm{.}20\backslash$times $10-3$ M$-1$s$-1$ at $700$ K$,$ determine the value of kf at the same temperature?Where kf is the forward reaction rate constant and kr is the reverse rate constant.$($c$)$ If the forward reaction is endothermic, explain with justification how an increase intemperature effects the values of Kc$,$ kf and kr$?$