ame: Page 3 (Question 1 continued) b) Determine the temperature at which this re

Question

ame: Page 3 (Question 1 continued) b) Determine the temperature at which this reaction will reach equilibrium. 2. The equilibrium reaction shown below has a standard Gibbs free energy change, AG, of -13.6 kJ/mol at 25°C. 2 NH3 (g) + CO2 (g) NH?CONH2 (aq) + H2O (e) a) Calculate Keq at this temperature. Keq = - b) Is this reaction predicted to be predominately products or reactants at equilibrium under standard conditions? Comment on the sign of AGº and the magnitude of Keq. Provide an explanation, rather than just stating a rule and use complete sentences.

Explanation / Answer

(a)
Fromula,

deltaG0 = - R TlnKeq

- 13.6 = - 0.008314 * 298.15 * lnKeq

lnKeq = 1.36 / (0.008314 * 298.15)

lnKeq = 0.549

Keq = e(0.549)

Keq = 3.54

(b)

Since deltaG0 is negative the reaction is product favoured. So at equilibrium the amounts of products is more than that of reactants.

But, the magnetude of Keq is 3.54, which is small enough, hence though products are more at equilibrium, the difference is not that much high.

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