a. Complete and balance: CaO( s ) + HNO 3 ( aq ) b. Calculate delta H o for the

Question

a. Complete and balance: CaO(s) + HNO3(aq)

b. Calculate delta Ho for the reaction in part a.

c. Calculate delta So for the reaction in part a.

d. Show how you would calculate delta Go for the reaction in part a. Plug all of the numbers into the appropriate equation, explicitly using the values you would plug into a calculator, if you had one available.

e. Predict the spontaneity of the reaction in part a. Briefly explain your reasoning.

f. Calculate the equilibrium constant using the data you calculated above. Is K greater than or less than one? Did you expect this value? Why or why not?

Substance

Delta Hof (kJ/mol)

So (J/mol

Substance

Delta Hof (kJ/mol)

So (J/mol

Explanation / Answer

a) CaO(s) + 2 HNO3(aq) = Ca(NO3)2(aq) + H2O(l)

b)   delta H0 = delta H0(product) - delta H0(reactant)

                      = (-543 -285.8) - ( -635.1 - 2 * 207.4) = 221.1 kJ/mol

c) delta S0 = delta S0(product) - delta S0(reactant)

                     = (-55.2 + 69.9) - ( 39.8 + 2 * 146.4) = - 317.9 J/mol.k

d)   delta G0 = delta H0 - T * delta S

                      = (221.1 kJ/mol) * 1000 - 298 * (- 317.9 J/mol.k) = 315.834 kj/mol

e) since delta G0 for the reaction is highly positve and for the reaction to be spontaneous delta G0 should be less than 0.so, the reaction will move in forward direction to achieve equilibrium.

f) delta G0 = -R* T * ln K  

=> 315.834 = - 8.314 * 298 * ln K

=> ln K = - 0.127 => k = 0.8807

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