For a phase change, h = -44 kj/mol and so = -0.12 kj/(k•mol). what are g and the spontaneity of the phase change at 350 k?

ΔG = - 2.0 kJ/mol and the reaction is spontaneous.

Explanation:

∵ ΔG = ΔH - TΔS,

ΔH = - 44.0 kJ/mol, T = 350.0 K, ΔS = - 0.12 kJ/K.mol.

∴ ΔG = ΔH - TΔS = (- 44.0 kJ/mol) - (350.0 K)(- 0.12 kJ/K.mol) = - 2.0 kJ/mol.

The sign of ΔG assigns the spontaneity of the reaction:

∵ ΔG has a negative value, so the reaction is spontaneous.

ΔG = - 2.0 kJ/mol and the reaction is spontaneous.

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.