Consider the following reaction and its Δ?∘Δ⁢G∘ at 25.00 °C. Fe2+(aq)+Zn(s)⟶Fe(s)+Zn2+(aq)Δ?∘=−60.73 kJ/molFe2+⁢(aq)+Zn(s)⟶Fe(s)+Zn2+⁢(aq)⁢Δ⁢G∘=−60.73 kJ/mol Calculate the standard cell potential, ?∘cell,Ecell∘, for the reaction. ?∘cell=Ecell∘=   V Calculate the equilibrium constant, ?,K, for the reaction. ?=K=

Calculate ΔrH° for the combustion of methane gas, CH4 : CH4(g)  +   2 O2(g)  →   CO2(g)  +  2 H2O(g) using standard molar enthalpies of formation: molecule                                  ΔfH° (kJ/mol) CH4(g)                                          -74.6 CO2(g)                                          -393.5 H2O( g)                                         -241.8   a) -802.5 kJ b) -495.2 kJ c) +802.5 kJ          d) -1460.3 kJ      e) -1828.5 kJ Group of answer choices

Calculate the temperature, in Kelvins, at which the decomposition of calcium carbonate becomes spontaneous (you do not need to include temperature units in your answer): CaCO3 (s) --> CaO (s) + CO2 (g) ΔHo = 179.0 kJ ΔSo = 160.2 J/K

Calculate ΔH° for the reaction:  2HNO3(l) → N2O5(g) + H2O(l)