Asked by Richard
The following questions relate to the chemical equation shown below. Since this is a multi-stage question, be sure to write down the balanced equation and the values for deltaHo and deltaSo before proceeding.
A2(g) + 3 B2(g) → 2 AB3(g)
deltaHo = -217 kJ mol-1
deltaSo = -199 J K-1 mol-1
Using the data provided, calculate the value of the standard free-energy change, deltaGo, for the reaction at 828 K.
A2(g) + 3 B2(g) → 2 AB3(g)
deltaHo = -217 kJ mol-1
deltaSo = -199 J K-1 mol-1
Using the data provided, calculate the value of the standard free-energy change, deltaGo, for the reaction at 828 K.
Answers
Answered by
DrBob222
dHrxn = (n*dHo products) - (n*dHo reactants)
dSrxn = (n*dSo products) - (n*dSo reactants)
dGrxn = dH - TdS
Post your work if you get stuck.
dSrxn = (n*dSo products) - (n*dSo reactants)
dGrxn = dH - TdS
Post your work if you get stuck.
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