Question

For a certain reaction, AGⓇ = -45 kJ/mol
and AH = -90 kJ/mol at 0 °C. What is
the minimum temperature at which
the reaction will become spontaneous,
assuming that AHⓇ and ASE
independent of temperature?
are
(a) 273 K
(b) 298 K
(c) 546 K
(d) 596 K​

Answer 1

Answer:

I didn't say the answer

Answer 2

Answer:

At constant temperature and pressure, the change in Gibbs free energy is defined as Δ G = Δ H − T Δ S \Delta \text G = \Delta \text H - \text{T}\Delta \text S ΔG=ΔH−TΔSdelta, start text, G, end text, equals, delta, start text, H, end text, minus, start text, T, end text, delta, start text, S, end text