I don't know to do ii) for letter a, as well as letter d, e and the EC . Can you help?
The combustion of carbon monoxide is represented by the equation below:
CO(g) + ½O 2 (g) → CO 2 (g)
(a) (i) Determine the value of the standard enthalpy change, ΔH
o 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 the
reactants 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 , for
the reaction at 298 K. Include units with
your answer. (3 pts)
ii) Is the reaction spontaneous under standard conditions at 298 K? Justify your answer. (2 pts)
(d) Calculate the value of the equilibrium constant, K eq , for the reaction at 298 K. (3 pts)
(e) Assume ∆H o and ∆S o for the reaction are independent of
temperature.
(i) Explain why there is a temperature above 298 K at which the
algebraic sign of the value of
∆G o changes. (2 pts)
(ii) Theoretically, the best yield of CO 2 should be achieved at
low temperatures or high
pressures. Explain each. (hint: apply Le Chatelier’s principle) (2
pts)
EC a) Write a net ionic equation for: Lithium metal is strongly heated in nitrogen gas. (2 pts)
b) Predict the sign of ΔS° for the reaction at 25°C. Justify your prediction. (1 pt)
A) A reaction has an equilibrium constant of Kp=0.280 at 44 ∘C. Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 3.35 kJ -3.35 kJ 0.404 kJ 0.466 kJ B) Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH= -11.0 kJ; ΔS = -17.4 J/K Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) = -11.0 kJ; = -17.4...
I need someone to show me how to solve thus problem, I think I have the right idea, but I may be plugging in something wrong. What is ΔS° at 298 K for the following reaction? Fe2O3(s)+ 3CO(g)→ 3CO2(g) + 2Fe(s) Substance ΔG°f(kJ/mol) ΔH°f(kJ/mol) Fe2O3(s). -741.0 -822.2 CO(g) -137.2 -110.5 CO2(g) -394.4 -393.5 Thanks
Consider the following reaction: 2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K Assume that all reactants and products are in their standard states. Calculate the free energy change for the reaction at 34 ∘C. Express your answer using four significant figures.
A reaction has an equilibrium constant of Kp=0.061 at 27 ∘C. Part A Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 6.98 kJ 0.839 kJ -6.98 kJ 0.628 kJ Part B Above what temperature does the following reaction become nonspontaneous? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = -1036 kJ; ΔS = -153.2 J/K 298 K 158.7 K 6.762 × 103 K This reaction is nonspontaneous at all...
2. For the following example, identify the following. H2O(l) → H2O(s) question 2 options a negative ΔH and a negative ΔS a positive ΔH and a negative ΔS a negative ΔH and a positive ΔS a positive ΔH and a positive ΔS It is not possible to determine without more information. 3. Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction. C2H2(g) + H2(g) → C2H4(g) S°(J/mol∙K) 200.9 130.7 219.3 Question 4 options:...
2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K For this problem, assume that all reactants and products are in their standard states. Calculate the free energy change for the reaction at 17 ∘C. Express your answer using four significant figures. ΔG = _____kJ
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: ΔH∘rxn=ΔH∘f(products)−ΔH∘f(reactants) Entropy change, ΔS∘, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free...
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: ΔH∘rxn=ΔH∘f(products)−ΔH∘f(reactants) Entropy change, ΔS∘, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free...
2Ca(s)+O2(g) → 2CaO(s) ΔH∘rxn= -1269.8 kJ; ΔS∘rxn= -364.6 J/K For this problem, assume that all reactants and products are in their standard states. Calculate the free energy change for the reaction at 29 ∘C. Express your answer using four significant figures. Part A ΔG = ______ kJ Part B Is the reaction spontaneous? spontaneous OR nonspontaneous
5. The standard molar entropy of liquid ethanol (C2H5OH) is 160.7 J K mol and the standard enthalpy of combustion is - 1368 kJ mol at 298 K, how much is the standard Gibbs energy (A,Gº) of formation of liquid ethanol at 298 K? (20 pts) The formation reaction of ethanol is 2C (graphite) + O2(g) + 3H2 (g) → C2H5OH() The combustion reaction of ethanol is CH5OH (1) + 302 (9) ► 200, (g) + 3H20 (1) CO; (g)...