JA H;º of H2O(1) is -285.8 kJ/mol. calculate A H° of MgO. The relevant reactions for these two heats of formation are: H2(g) + ½ O2(g) → H20(1) and Mg(s) + ½ O2(g) – MgO(s) -141.3 kj/mol a) b) -306.6 kj/mol c) -447.9 kj/mol d) -592.4 kj/mol e) 141.3 kj/mol f) Not even information given

Using the given bond dissociation energies, calculate H°rxn for the following reaction:2 H – Cl(g) + Br – Br(g)  2 H – Br(g) + Cl – Cl(g) A. + 78 kJB. - 308 kJC. + 14 kJD. + 564 kJBE (kJ/mol)H – Cl: 427H – Br: 363Cl – Cl: 243Br – Br: 193

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What is the AH°rxn for the reaction of gaseous ammonia and oxygen gas to form gaseous nitrogen monoxide and water vapor? Use the given standard heats of formation. Write the balanced chemical reaction. AH°; NH3 (g) AH°;02 (g) = 0 AH°;NO (g) = 103.56 kJ/mol AH°; H20 (g) = -218.42 kJ/mol = -38.17 kJ/mol %3D

Calculate the AH°, for the reaction below, in kJ, using the heat of formation values below: _X4Y2 (g) + Z, (g)→ --_X2Z4 (g) + LY4Z2 () AH°; [X4Y2 (g)] = -300.5 kJ/mol AH°; [Z, (g)] = O k//mol AH°; [X2Z4 (g)] = -110.4 kJ/mol AH°; [Y4Z2 (] = 278.9 kJ/mol %3D HINT: Balance the reaction FIRST!

Methane-producing bacteria convert liquid acetic acid (CH3CO₂H) into CO₂(g) and CH₂(g). AS° ΔΗ, Ο (kJ/mol) (J/mol.K) CH3CO₂H (1) -484.5 159.8 CO₂(g) -393.5 213.8 CH₂(g) -74.8 186.2 Calculate AHOrxn = kJ Calculate AG rxp = (round to 3 sig figs) Is this process endothermic or exothermic under standard conditions? Is the reaction spontaneous under standard conditions? kJ (round to 3 sig figs)

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Can someone verify my answers? I got: a)  endothermic b)-1149.5 J c) 1149.5 J d)0.0117 mol e) 97704.05 J/mol

Methane-producing bacteria convert liquid acetic acid (CH³CO₂H) into CO₂(g) and CH₂(g). AS° ΔΗ, Ο (kJ/mol) (J/mol.K) CH3CO₂H (1) -484.5 159.8 CO₂(g) -393.5 213.8 CH₂(g) -74.8 186.2 Calculate AHºrxn = kJ Calculate AG, = rxn (round to 3 sig figs) Is this process endothermic or exothermic under standard conditions? Is the reaction spontaneous under standard conditions? kJ (round to 3 sig figs)

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