Calculate `Delta_(r)G` for the reaction at `27^(@)C`
`H_(2)(g) + 2Ag^(+)(aq) implies 2Ag(s) + 2H^(+)(aq)`
Given : `P_(H_2) = 0.5 , [Ag^+] = 10^(-5)M`,
`[H^+] = 10^(-3) M , Delta_(f) G^(@) [Ag^(+)(aq)]`
`= 77.1 kJ//mol`

Calculate Delta_(r)G^(c-) of the reaction : Ag^(o+)(aq)+Cl^(c-)(aq) rarr AgCl(s) Given :Delta_(f)G^(c-)._(AgCl)=-109kJ mol ^(-1) Delta_(f)G^(c-)_((Cl^(c-)))=-129k J mol ^(-1) Delta_(f)G^(c-)._((Ag^(o+)))=-77 kJ mol ^(-1)

The cell reaction 2Ag^+(aq)+H_2(g)to2H^+(aq)+2Ag(s) ,best represented by :

Calculate Delta_(r) H^(@) for Fe_(2) O_(3) (s) + 3 CO(g) to 2 Fe (s) + 3 CO_(2) (g) Given : Delta_(f) H^(@) (Fe_(2) O_(3) , s) = -822.2 kJ/mol Delta_(f) H^(@) (CO , g) = -110.5 kJ//mol , Delta_(f) H^(@) (CO_(2) , g) = -393.5 kJ/mol

The reaction, (1)/(2) H_(2) (g) + Ag Cl (s) = H^(+) (a.q) + Cl^(-) (a.q) + Ag (s) occurs in the galvanic cell:

The reaction, (1)/(2)H_(2)(g) + AgCl(s) H^(+)(aq)+Cl^(-) (aq)+Ag(s) . Occurs in the galvanic cell :