The standard enthalpy of formation of gaseous `H_(2)O` at 298 K is `-241.82` kJ/mol. Calculate `DeltaH^(@)` at 373 K given the following values of the molar heat capacities at constant pressure : `H_(2)O(g)=33.58 " JK"^(-1)" mol"^(-1), " "H_(2)(g)=29.84 " JK"^(-1)" mol"^(-1), " "O_(2)(g)=29.37 " JK"^(-1)" mol"^(-1)` Assume that the heat capacities are independent of temperature :
A
`-242.6 kJ//mol`
B
`-485.2 kJ//mol`
C
`-121.3 kJ//mol`
D
`-286.4 kJ//mol`
Text Solution
Verified by Experts
The correct Answer is:
A
`Delta_(r )C_(p)^(@)=-10.945" for"` `H_(2)(g)+(1)/(2)O_(2)(g)rarrH_(2)O(g)` According to Kirchhoff's law `Delta_(r )H_(T_(2))^(@)-Delta_(r )H_(T_(1))^(@)=Delta_(r )C_(p)^(@)[T_(2)-T_(1)]` `Delta_(r )H_(T_(2))^(@)-(241.82)=[-10.94 J (373-298)//100]` `implies Delta_(r )H_(T_(2))=-242.6 " kJ"//"mol"`
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