@X@user.full_name@X@ @GMU: From the reaction below, calculate the free energy of formation for C7H16(g) at 25°C, if ΔGfo(CH4(g)) is -50.790 kJ/mol.7CH4(g) → C7H16(g) + 6H2(g) ΔGo = 364.105 kJ/mol

@X@user.full_name@X@ @GMU: What is the empirical formula of a compound if its percent composition is 68.74% C and 12.18% H and 8.907% N ? The compound contains only C, H, N and O.

@X@user.full_name@X@ @GMU: What is the free energy change at 25°C for the reaction below, if ΔGfo(CH4(g) = -50.790 kJ/mol, ΔGfo(C5H12(g)) is -8.234 kJ/mol.C5H12(g) + 4H2(g) → 5CH4(g)

@X@user.full_name@X@ @GMU: What is the energy of a photon having a wavelength of 28.47 pm? Remember Planck’s constant is 6.626×10-34 J×s

@X@user.full_name@X@ @GMU: What is the balanced reaction for the following galvanic cell?Cd(s)| Cd2+(aq) || Pb2+(aq) | Pb(s)

@X@user.full_name@X@ @GMU: What is the wavelength of photons having an energy of 0.0760 kJ/mol. Remember Planck’s constant is 6.626×10-34 J×s

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@X@user.full_name@X@ @GMU: From the reaction below, calculate the free energy of formation for C9H10(g) at 25°C, if ΔGfo(CH4(g)) is -50.790 kJ/mol.9CH4(g) → C9H10(g) + 13H2(g) ΔGo = 665.845 kJ/mol

@X@user.full_name@X@ @GMU: A gas mixture contains an unknown amount of CH4 and 0.0907 mol of HCN. How many moles of CH4 are there, if the total pressure is 692.06 mm Hg and the partial pressure of CH4 is 418.25 mm Hg?

@X@user.full_name@X@ @GMU: ACS-What is ΔG° for the reaction below, if ΔH° = 98.80 kJ, ΔS° = 141.500 J/KFe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(g)