I don't know to do ii) for letter a, as well as letterd, e and the EC . Can you help?

The combustion of carbon monoxide is represented by the equationbelow:

CO(g) + ½O 2 (g) → CO 2 (g)

(a) (i) Determine the value of the standard enthalpy change, ΔHo rxn, for the combustion of CO(g) at
298 K using the following information. (3 pts)

C(s) + ½O 2 (g) → CO(g) ΔH o 298 = -110. 5 kJ mol -1
C(s) + O 2 (g) → CO 2 (g) ΔH o 298 = -393.5 kJ mol -1

(ii) Which is larger, the total bond dissociation energy of thereactants or the total bond
dissociation energy of the products? Explain. (2 pts)

(b) Determine the value of the standard entropy change, ΔS o rxn, for the combustion of CO(g) at 298
K using the information in the following table. (3 pts)
Substance S o 298(J mol -1 K -1 )
CO(g) 197.7
CO 2 (g) 213.7
O 2 (g) 205.1

(c) i) Determine the standard free energy change, ΔG o rxn , forthe reaction at 298 K. Include units with
your answer. (3 pts)

ii) Is the reaction spontaneous under standard conditions at 298K? Justify your answer. (2 pts)

(d) Calculate the value of the equilibrium constant, K eq , forthe reaction at 298 K. (3 pts)

(e) Assume ∆H o and ∆S o for the reaction are independent oftemperature.
(i) Explain why there is a temperature above 298 K at which thealgebraic sign of the value of
∆G o changes. (2 pts)

(ii) Theoretically, the best yield of CO 2 should be achieved atlow temperatures or high
pressures. Explain each. (hint: apply Le Chatelier’s principle) (2pts)

EC a) Write a net ionic equation for: Lithium metal is stronglyheated in nitrogen gas. (2 pts)

b) Predict the sign of ΔS° for the reaction at 25°C. Justifyyour prediction. (1 pt)