What is the Gibbs free energy of methane?
=−74.8 kJ−298 K⋅−0.0809 kJ/K. =−50.68 kJ/mol→−50.7 kJ/mol.
What is the standard Gibbs free energy change for the combustion of methane?
ΔS° = -0.2422 kJ K-1mol-1. This reaction is actually the combustion of methane, and so we can just take a value of this from a Data Book.
What is the Gibbs free energy at 298 K for the formation of methane?
The standard enthalpy of formation (ΔfH°) at 298 K for methane, CH4(g), is –74.8 kJ mol–1.
Which substance has zero Gibbs free energy of formation?
Fluorine
Standard Gibbs free energy of formation
| Species | Phase (matter) | ΔGf° (kJ/mol) |
|---|---|---|
| Fluorine | Gas | 0 |
| Hydrogen | ||
| Hydrogen | Gas | 0 |
| Water | Liquid | −237.14 |
What is Delta S of CH4?
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ∆H = -890.3 kJ. ∆S = -242.6 J/K = – 0.2426 kJ/K. m = –∆S = +0.2426 kJ/K.
How do you calculate delta G standard?
ΔG=ΔG0+RTlnQ where Q is the ratio of concentrations (or activities) of the products divided by the reactants. Under standard conditions Q=1 and ΔG=ΔG0 . Under equilibrium conditions, Q=K and ΔG=0 so ΔG0=−RTlnK . Then calculate the ΔH and ΔS for the reaction and the rest of the procedure is unchanged.
What does a positive change in Gibbs free energy mean?
Reactions with a negative ∆G release energy, which means that they can proceed without an energy input (are spontaneous). In contrast, reactions with a positive ∆G need an input of energy in order to take place (are non-spontaneous). Reactions with a positive ∆H and negative ∆S are non-spontaneous at all temperatures.
What is the ΔFH value for o2 G in kJ mol?
0 kJ/mol
The relevant standard enthalpy of formation values from Table 1 are: O2(g): 0 kJ/mol.