Question

The standard gibbs energy changes for the reaction
H2O--:H+* OH- at 25 degree celcius

Answer 1

Answer: 79882 Joules

Explanation:

Formula used :

$\Delta G^o=-2.303\times RT\times \log K_c$

where,

$\Delta G^o$ = Gibbs free energy = ?

R = universal gas constant = 8.314 J/K/mole

T = temperature = $25^0C=(25+273)K=298 K$

$H_2O\rightarrow H^++OH^-$

$K_w$ = equilibrium constant = ${[H^+][OH^-]}$ =$10^{-14}$

$\Delta G^o=-2.303\times 8.314\times 298\times \log(10^{-14})$

$\Delta G^o=+79882Joules$

Thus standard gibbs energy changes for the reaction is 79882 Joules