2. Calculate delta g for the dissolution of urea when 4.4 g of urea dissolved in

Question

2. Calculate delta g for the dissolution of urea when 4.4 g of urea dissolved in 4.7 ml of water at 25 degrees Celsius. R= 8.314 J/mol•k
3. Calculate delta s if delta g = 80.34 kJ/mole and delta h = 87 kJ/mole at 25 degrees Celsius 2. Calculate delta g for the dissolution of urea when 4.4 g of urea dissolved in 4.7 ml of water at 25 degrees Celsius. R= 8.314 J/mol•k
3. Calculate delta s if delta g = 80.34 kJ/mole and delta h = 87 kJ/mole at 25 degrees Celsius 2. Calculate delta g for the dissolution of urea when 4.4 g of urea dissolved in 4.7 ml of water at 25 degrees Celsius. R= 8.314 J/mol•k
3. Calculate delta s if delta g = 80.34 kJ/mole and delta h = 87 kJ/mole at 25 degrees Celsius Question 2 (10 points) Calculate for the dissolution of urea when 4.4 g of urea dissolved in 4.7 mL of water at 25 R-8.3143/me.K Your Answer Question 3 (10 points) Calculate as. if ?G. . 80.34 krmole and ?" " 87 k/mole at 25 °C, Your Answer Pr LR 3 8

Explanation / Answer

The first thing to do is to calculate the number of moles of Urea (aq) and the concentration of this (molar mass of urea is 60)

moles = mass / molar mass

moles = 4.4 / 60 = 0.0733 moles of urea

Molarity (volume of solution is 0.0047 L)

Molarity = moles / volume = 0.0733 / 0.0047 = 15.5957 M

Apply the equation

G = - RT ln Kc

where R is gas constant

T is temperature in kelvin

Kc is the equilibrium constant

for urea

Urea + H2O === Urea (aq)

kc = [Urea] , only urea is considered in the equilibrium equation so:

G = - 8.314 * 298.15 * 15.597 = - 38662.1415 J / mol , divide this by 1000 to get

G = - 3.866 Kj / mol

3. The relationship between Gibbs, entropy and enthalpy is :

G = H - T S, where G is gibbs energy

H is enthalpy

T is temperature

S is entropy

80.34 Kj / moles = 87 kj / mol - 298.15 * S

80.34 - 87 = -298.15 * S

-6.66 = -298.15 * S

S = 6.66 / 298.15 = 0.0223 Kj / mol, multiply this by 1000 to get:

S = 22.33 J / mole

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