Data: AH°¡ values: CH4(g), -74.8 kJ; CO2(g), -393.5 kJ; H20(1), -285.8 kJ. Using the AH° data above, calculate AH°rxn for the reaction below. Reaction: CH4(g) + 202(g) → + 2H20(1) CO2(g)

Using the following equations, N,0(g)– 2NO2(g) AH° = +57.93 kJ 2NO(g) + O(g) 2NO,(g) AH° = -113.14 kJ %3D calculate the AH° for the following reaction: 2NO(g) + O2(g)– N,0,(g) AH° = kJ

04) (g Calculate the volume of air at 30°C and 1.00 atm that is needed to burn completely 10.0 grams of propane. Assume that air is 21.0 percent O₂ by volume. The heat of combustion of propane is -2,220.1 kJ/molrxn. Calculate the heat of formati of propane given that AHO of H₂0(1) = -285.3 kJ/mol and AHO of CO2(g) = -393.5 kJ/ f AH-[(3•Co₂) + (4•H₂0)]-[C3H8 + 5(0₂)] [ F)+(4(-285.3)]-[AH C3H5] [200

Calculate AH for the following reaction: IXI C(s) +H,0(g)→Co(g) - H, (3) Use the following reactions and given AH values: C(s) + O2 (g)→CO, (g), AH- 393.5 kJ 20(g) + 02 (g)→2CO2(g), AH = -566.0 kJ 2H2 (g) + O2 (g)→2H2O(g). AH = -483.6 kJ Express your answer using four significant figures.

Use Hess's Law to calculate the enthalpy change for the reaction AH=? from the following data: 2BaO(s) -(0 + (S) AH3-1107.0kJ AH=-822.5kJ (s)E00 ( 04 + (O + (s) %3D O-284.5 kJ O 538.0 kJ O 1391.5 kJ Previous

Given the following information, AH° (A2B(g)) = -225 KJ/mol AH (BC(g)) = -160 KJ/mol %3D AH (AC(g)) = -85 KJ/mol AH (B(g)) = -75 KJ/mol Determine AH° for the reaction, A2B(g) + 2BC(g) 2AC(g) + 3B(g) -600 KJ/mol 150 KJ/mol 600 KJ/mol 450 KJ/mol

reaction W Calculate AG rxn For the following at 450k CH ₂0 (g) + 2H₂ (9) → CHH (g) + H₂O (9) Using AH = -94.9 KJ; A'S = -224.2J/K