$2\mathrm{.}9$ Consider the following hydrogen$$oxygen fuel cell reaction

H$2+1/2$O$2->$ H$2$O$($l$)$

at the standard temperature and pressure $(1$ atm and $25$C$).$ If the cell operates at the cell voltage of E$=0\mathrm{.}7$V$,$ then determine for each mole fuel consumed in the cell $($a$)$ the amount of electrical work done; $($b$)$ the amount of entropy

generation; $($c$)$ the amount of cell potential loss; $($d$)$ the amount of waste heat generation.

$2\mathrm{.}10$ Repeat the calculation from Problem $2\mathrm{.}9$ if the hydrogen$-$oxygen reaction occurs at $80$C and $1$ atm.

$2\mathrm{.}11$ Repeat the calculation from Problem $2\mathrm{.}9$ if the reaction occurs reversibly, instead of at the cell potential of E$=0\mathrm{.}7$V$,$ for the condition of

$($a$)25$C and $1$ atm,

$($b$)80$C and $1$ atm,

$($c$)80$C and $3$ atm.