We can use the following equation to solve for ΔG˚rxn:
For this problem, we need to do the following steps:
Step 1: Calculate ΔH˚rxn.
Step 2: Calculate ΔS˚rxn.
Step 3: Use ΔH˚rxn and ΔS˚rxn to calculate for ΔG˚rxn.
Step 1: We can use the following equation to solve for ΔH˚rxn:
Note that we need to multiply each ΔH˚f by the stoichiometric coefficient since ΔH˚f is in kJ/mol.
Also, note that ΔH˚f for elements in their standard state is 0.
Given the following information determine the reaction Gibbs energy for the formation of hydrazine (N2H4) at 298 K
2NH3(g) → N2H4(l) + H2(g)
NH3 : ΔH°f = -46.11 kJ mol-1 ΔS° = 192.45 J mol-1 K-1
N2H4 : ΔH°f = 50.63 kJ mol-1 ΔS° = 121.21 J mol-1 K-1
H2 : ΔH°f = 0 ΔS° = 130.7 J mol-1 K-1
Answer to TWO decimals places in kJ mol-1
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.