Why gibbs energy is more convinent to predict the direction of reaction?
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When a process occurs at constant temperature \text TTT and pressure \text PPP, we can rearrange the second law of thermodynamics and define a new quantity known as Gibbs free energy:
\text{Gibbs free energy}=\text G =\text H - \text{TS}Gibbs free energy=G=H−TSG, i, b, b, s, space, f, r, e, e, space, e, n, e, r, g, y, equals, G, equals, H, minus, T, S
where \text HHH is enthalpy, \text TTT is temperature (in kelvin, \text KKK), and \text SSS is the entropy. Gibbs free energy is represented using the symbol \text GGGand typically has units of \dfrac{\text {kJ}}{\text{mol-rxn}}mol-rxnkJstart fraction, k, J, divided by, m, o, l, negative, r, x, n, end fraction
When a process occurs at constant temperature \text TTT and pressure \text PPP, we can rearrange the second law of thermodynamics and define a new quantity known as Gibbs free energy:
\text{Gibbs free energy}=\text G =\text H - \text{TS}Gibbs free energy=G=H−TSG, i, b, b, s, space, f, r, e, e, space, e, n, e, r, g, y, equals, G, equals, H, minus, T, S
where \text HHH is enthalpy, \text TTT is temperature (in kelvin, \text KKK), and \text SSS is the entropy. Gibbs free energy is represented using the symbol \text GGGand typically has units of \dfrac{\text {kJ}}{\text{mol-rxn}}mol-rxnkJstart fraction, k, J, divided by, m, o, l, negative, r, x, n, end fraction
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