Under a constant pressure of 1.000atm, we do the combustion of 1.0000mol of propane, C3H8(g), at 25.0C (N.B. combustion is the reaction of a substance with O2(g) to produce CO2(g) and H2O(l)). Calculate the values of H,U,Q, and W for this combustion. If the combustion of 2.22mol of propane, C3H8(g), at constant pressure is used to heat 50.0 kg of water originally at 25.0C, what will be the final temperature of this 50.0kg of water? N.B. that R=0.082056L atm / mol K =8.3145J/molK. The enthalpies of formation of C3H8(g),CO2(g), and H2O(l) are 103.9,393.5, and 285.8kJ/mol, respectively. The specific heat of water is 4.184J/gK