Ask a New Question
Menu

I don't understand this one at all. Please help!

For the equation: MnO2 (s) + 2 CO (g) → Mn (s) + 2 CO2 (g)

1. Calculate ΔG° at 25°C

2. Calculate ΔG° at 125°C

1 answer

#1.
dGo rxn = (n*dGo products) - (n*dGo reactants)

#2. Are you sure you don't mean dG rxn at 125 C. I was always under the impression that dGo is the standard at 25C. This T is not 25 C and I would call it dG rxn and not dGo rxn
For that calculate dHo rxn = (n*dHo products) - (n*dHo reactants).
Do the same with dSo rxn.
Then dG rxn = dHrxn - TdS reaction. Remember dH usually given in kJ and dS in J so convert one or the other.
Similar Questions
  1. MnO4^-(aq) + H20(l) ==> MnO2 + OH^-net charg is -1 +7 (-8) ==> 4(-4) Manganese is reduced MnO4^- +3e- ==> MnO2 H2) is the
    1. answers icon 2 answers
  2. Consider the reaction MnO2+4HCL===>MnCl2+Cl2+2H2OHow many grams of MnO2 are required to produce 5.6 of Cl2 at stp?MnO2=87
    1. answers icon 1 answer
  3. For the equation: MnO2 (s) + 2 CO (g) → Mn (s) + 2 CO2 (g)Calculate ΔG at 298K if MnO2 = 0.150 mol, Mn = 0.850 mol, CO =
    1. answers icon 1 answer
    1. answers icon 1 answer
more similar questions