Balancing the Combustion Equation
One kmol of octane \left(\mathrm{C}_{8} \mathrm{H}_{18}\right) is burned with air that contains 20 \mathrm{kmol} of \mathrm{O}_{2}, as shown in Fig. 15-7. Assuming the products contain only \mathrm{CO}_{2}, \mathrm{H}_{2} \mathrm{O}, \mathrm{O}_{2}, and \mathrm{N}_{2}, determine the mole number of each gas in the products and the air-fuel ratio for this combustion process.