Answer:
286 J/K
Explanation:
The molar Gibbs free energy for the vaporization (ΔGvap) is:
ΔGvap = ΔHvap - T.ΔSvap
where,
ΔHvap: molar enthalpy of vaporization
T: absolute temperature
ΔSvap: molar entropy of the vaporization
When T = Tb = 64.7 °C = 337.9 K, the reaction is at equilibrium and ΔGvap = 0.
ΔHvap - Tb . ΔSvap = 0
ΔSvap = ΔHvap/Tb = (71.8 × 10³ J/K.mol)/ 337.9 K = 212 J/K.mol
When 1.35 mol of methanol vaporizes, the change in the entropy is:
Answer:
The correct answer is A
Explanation:
Endothermic is a reaction of which heat is provided to break down the reacted molecules
Answer:
Dilute
Explanation:
Henry's law
This is a physical chemistry law , according to which , in a dilute solution , i.e. , with less concentration of solute , the amount of the dissolved gas in the liquid is directly proportional to its partial pressure above the liquid .
Henry's law constant is the proportionality constant .
The application of Henry's law is , the carbonated soft drinks , which have dissolved carbon dioxide .i.e. ,
By increasing the pressure , the solubility of the gas also increases .
Answer:
the answer is c- convection only
Explanation:
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