// Given:-
// When expressed on a per mole of fuel basis, the balanced chemical equation obtained in the solution to Example 13.2  takes the form
// CH4 + 2.265O2 + 8.515N2  -----  .951CO2 + .049CO + .289O2 + 8.515N2 + 2H2O
cpbar = 38.00                                                                   // specific heat in KJ/kmol.K
// From table A-25
hfnotbar = -74850.00                                                            // enthalpy of formation for methane
// From table A-23
deltahbarO2 = 14770-8682
deltahbarN2 = 14581-8669

// Calculations
hRbar = hfnotbar + cpbar*(400-298) + 2.265*deltahbarO2 + 8.515*deltahbarN2      // in kj/kmol
// With enthalpy of formation values for CO2, CO, and H2O(g) from Table A-25 and enthalpy values from Table A-23
hpbar = .951*(-393520 + (88806 - 9364)) + .049*(-110530 + (58191 - 8669)) + .289*(60371 - 8682) + 8.515*(57651 - 8669) + 2*(-241820 + (72513 - 9904))
Qcvdot = hpbar - hRbar                                                          // in kj/kmol

// Result
printf( ' The rate of heat transfer from the combustion chamber in kJ per kmol of fuel is:  %.2f',Qcvdot)