Question

In a laboratory experiment 78.612 g of methane is burned in air containing O2 to form gaseous CO2 and H2O. Calculate the final temperature in °C of the product mixture if the methane and air are both at an initial temperature of 4.9°C. Assume a stoichiometric ratio of methane to oxygen from the air, with air being 21% O2 by volume and the rest of the volume being N2 (c of CO2 = 57.2 J/molK; c of H2O(g) = 36.0 J/molK; c of N2 = 30.5 J/molK). Use data of formation enthalpies from the appendix if needed. Enthalpies: CO2(g): -393.5 kJ/ mol, H2O(g): -241.826 kJ/ mol, O2(g): 0 kJ/ mol, N2(g): 0 kJ/ mol, CH4(g): -74.87

Answer 1

I hope this helps you.If you find any problem please comment on below and gives a thumbs up if you like it.

duced= 4'9 m a produced CH2