Date:Equilibrium Constant $-$ Calculations$1.$ Write the equilibrium expression for the following reactions:a$.$b$.$c$.$d$.$e$.$f$.$g$.2.$ Consider the following equilibrium reaction:The Keq for this reaction at $25$ is $1\mathrm{.}02.$ At equilibrium the concentration of HBr is $0\mathrm{.}50$mol$/$L$.$ Assuming H$2$ and Br$2$ are present in equal amounts, calculate the concentration of H$2$ at equilibrium. $3.$ Analysis of the following equilibrium reaction at $900$ provides the concentrations listed below:Experiment$[$H$2$O$][$CO$][$H$2][$CO$2]10\mathrm{.}3520\mathrm{.}3520\mathrm{.}1480\mathrm{.}64820\mathrm{.}2660\mathrm{.}2660\mathrm{.}2340\mathrm{.}23430\mathrm{.}6860\mathrm{.}1860\mathrm{.}3140\mathrm{.}314$Write the equilibrium expression for the reaction and calculate the value of the equilibrium constant for each experiment. $4.$ In the following reaction at $448,$ the equilibrium concentrations are HI $=0\mathrm{.}0040$M$,$ H$2=0\mathrm{.}0075$M$,$ I$2=0\mathrm{.}000043$M$.$ Calculate the equilibrium constant given the reaction below: $5.$ If the temperature of an exothermic reaction at equilibrium is lowered, is the value of Keq increased or decreased?