a.
C(s) + O2 ==> CO2
dHfrxn = (n*dHf products) - (n*dHf reactants)
Then
dHfrxn in kJ/mol x (#mols) = 1000 kJ
Solve for # mols.
The others are done the same way but the eq2uation is combustion equation isn't quite as simple as CO2.
Use enthalpy of formation data to calculate the number of moles of CO2(g) produced per megajoule of heat released from the combustion of each fuel under standard conditions (1atm and 25 degrees C)
a. coal C(s, graphite) = _____mole-MJ
b. natural gas, CH4(g)=
c. propane, C3H8(g)=
d. octane, C8H18(l) (H(f)= -250.1kJ)=
2 answers
Could you do the first one for me so I can see please?
4 answers