Calculate DeltaSdegree_rxn, (in J/K), DeltaHdegree_rxn(in kJ), and DeltaGdegree

Question

Calculate DeltaSdegree_rxn, (in J/K), DeltaHdegree_rxn(in kJ), and DeltaGdegree (in kJ) for each of the following reactions at 25.0 degreeC. Refer to the Appendix in your textbook for thermodynamic data. a. NO_2(g) + NO_2(g) rightarrow 3NO(g) b. 4NH_3(g) + 5O_2(g) rightarrow 4NO(g) + 6H_2O(I) c. 2C_2H_6(g) + 7O_2(g) 4CO_2(g) + 6H_2O(g) d. CaCO_3(s) + 2HCI(aq) CaCI_2(aq) + H_2O(I) + CO_2(g) e. 6CO_2(g) + 6H_2O(I) rightarrow C_6H_12O_6(s) + 6O_2(g) 2. Chloroform, CHCI_3, is an organic solvent and has been used as an anesthetic. The heat of vaporization of chloroform at its boiling point (61.2degreeC) is 29.6 kJ/mol. What is the entropy change when 1 mole of chloroform vaporizes at its boiling point? DeltaG = 0 at the boiling point since the process is at equilibrium at this temperature.

Explanation / Answer

1) delta H0rkn = (delta H0f of products) - (delta H0f of reactants)

delta S0rkn = (delta S0f of products) - (delta S0f of reactants)

delta G0rkn = delta H0rkn - T*delta S0rkn

2) delta G = delta H - T*delta S

Now, delta G = 0

Thus , delta S = delta H/T = 29600/(273+61.2) = 88.57 J/K

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