Home
Class 12
CHEMISTRY
The standard enthalpy of formation of ga...

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 :

Promotional Banner

Similar Questions

Explore conceptually related problems

The standard enthalpy of formation of H_2O(g) at 298 K is -241.82 kJ mol^-1 , Calculate DeltaH^@ at 373 K. Assume that C_p , is independent of temperature C "_p^o of H_2O(g) = 33.58 JK^-1 mol^-1 C "_p^o of H_2(g) = 28.84 JK^-1 mol^-1 C "_p^o of O_2(g) = 29.37 JK^-1 mol^-1

The standard enthaply for the reaction H_(2)(g) + 1//2 O_(2)(g) to H_(2)O(l) is - 285.76 kJ at 298 K. Calculate the value of DeltaH at 373 K .The molar heat capcities at constant pressure (C_(P)) in the given temperature range of H_(2)(g),O_(2)(g) and H_(2)O(l) are respectively 38.83,16 and 75.312 JK^(-1) mol^(-1) .

The standard enthalpies of formation of H_(2)O(l) and CO_(2)(g) are respectively -286" kJ mol"^(-1) and -394" kJ mol"^(-1) . If the standard heat of combustion of CH_(4)(g)" is "-891" kJ mol"^(-1) , then the standard enthalpy of formation of CH_(4)(g) is

S_(H_(2(g)))^(0) = 130.6 JK^(-1) mol^(-1), S_(H_(2)O_((l)))^(0) = 69.9JK^(-1) mol^(-1), S_(O_(2(g)))^(0) = 205 JK^(-1) , Then the absolute entropy change of H_(2(g)) + (1)/(2)O_(2(g)) rarr H_(2)O_((l)) is