Answer: The equilibrium constant for the reaction at 25 °C is 346.7
Explanation:
Formula used :
where,
= standard Gibb's free energy change = -14.50kJ/mol =14500 J/mol
R = universal gas constant = 8.314 J/K/mole
T = temperature =
= equilibrium constant = ?
Putting in the values we get:
The equilibrium constant for the reaction at 25 °C is 346.7
Answer:- solution boiling point = 102.23 degree C (102 degree C with three sig figs).
Solution:- When a non volatile solute is added to a solvent then boiling point increases. Elevation in boiling point is directly proportional to the molality of the solution.
The equation is:
where, is the elevation in boiling point, i is the Van't hoff factor,
is the molal elevation constant and m is the molality.
Value of i is 1 as ethylene glycol is a covalent molecule that does not break to give ions. for water is
.
We can calculate the molality from the given grams of ethylene glycol and liters of water as molality is moles of solute per kg of solvent.
Molar mass of ethylene glycol is 62 gram per mol and density of water is 1.00 kg per liter.
= 2.50 kg
Let's calculate the moles of ethylene glycol.
= 10.9 mol
molality of the solution =
= 4.36m
Let's plug in the values in the equation we have on the top for elevation in boiling point.
=
Boiling point of pure water is 100 degree C. So, the boiling point of the solution = 100 + 2.23 = 102.23 degree C
(If we fix the three sig figs then it could be written as 102 degree C.)