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Using the table of standard entropies and enthalpies of formation, calculate AH°, ASº, and AG° for...
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table...
(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table provided, calculate the enthalpy of reaction ΔH°rxn (in kJ) for each of the following reactions: Standard Enthalpies of Formation substance ΔHf° in kJ/mol Mg(s) 0 MgO(s) -601.6 HCl(aq) -167.2 MgCl2(aq) -801.2 H2(g) 0 H2O(l) -285.8 Reaction #1: Mg (s) + 2HCl (aq) è MgCl2 (aq) + H2 (g) Reaction #2: MgO (s) + 2HCl (aq) è MgCl2 (aq) + H2O (l) 2. (4 pts.)...
Use standard enthalpies of formation (in Appendix G in text) to calculate ∆H°rxn for each reaction. ...
Use standard enthalpies of formation (in Appendix G in text) to calculate ∆H°rxn for each reaction. ∑ m∆H°f (products) - ∑n∆H°f (reactants), where m and n are coefficients. C2H4(g) + H2(g) ----- > C2H6(g) CO (g) + H2O (g) ----- > H2(g) + CO2(g) 3NO2(g) + H2O (l) ----- > 2HNO3(aq) + NO (g) 2SO2(g) + O2(g) -----------> 2SO3(g) 2C4H10 (g) + 13O2 (g) -----------> 8CO2 (g) + 10H2O (g) Substance --- ΔH° (kJ mol–) --- ΔG° (kJ mol–1) --- S°298 (J K–1 mol–1) C2H4 52.4 86.4 219.3 H2 0 0 130.7 C2H6 -84.0 -32.0 229.2 CO -110.52 -137.15 197.7 H2O -285.83 -237.1 70.0 CO2 -393.51 -394.36 213.8 NO2 33.2 51.30 240.1 NO 90.25 87.6 210.8 SO2 -296.83 -300.1 248.2 O2 0 0 205.2 SO3 -395.72 -371.06 256.76
Calculate the standard enthalpy of formation of gaseous sulfur dioxide (S02) using the following thermochemical information:...
Calculate the standard enthalpy of formation of gaseous sulfur dioxide (S02) using the following thermochemical information: 2 Mgo(s) = 2 Mg(s) + O2(g) Mg(s) + S(s) = MgS(s) Mgs(s) + 2 Mgo(s) = 3 Mg(s) + SO2(g) AH = +1203.4 k) AH = -598.0 kJ AH = +1504.6 kJ AH = k]
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous...
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous carbon dioxide and liquid water at 25 °c (AHe AH/kJ mol 393.5 -285.9 -1559.7 C(graphite) H2(g) C2Ho(g) 5.9 131.0 229.5 Calculate the enthalpy change (AH) and Gibbs energy change (AG) for the reaction 2C(graphite) +3H28)CH) datseatt Is this reaction thermodynamically possible? Give a reason for your answer. (10 marks) Explain why it is possible for endothermic processes to occur spontaneously. 15 marks]
Calculate [delta H0 f] in kJ for the equation below using the standard enthalpies of formation...
Calculate [delta H0 f] in kJ for the equation below using the
standard enthalpies of formation seen in the image:
Testbank, Question 6.123 Using the standard enthalpies of formation, AH : CO(g) = -110.5 kJ mol-1 CO2(g) = -393.5 kJ molt SO2(g) = -296.9 kJ molt SO3(g) = -395.2 k) mol-1 calculate AH reaction for CO2(g) + SO2(g) — 503(9) + CO(g)
10. (10 points) Use standard enthalpies of formation listed in the attached table to find AH°...
10. (10 points) Use standard enthalpies of formation listed in the attached table to find AH° values for the following reaction at 25°C. NH3(g) + HCl(g) + NH4Cl (s) Substance NH3(g) HCl(g) NHACI (s) AH f (kJ/mol) -45.9 -92.31 -314.43 Is the reaction endothermic or exothermic?
c) The standard enthalpies of formation and molar entropies of phosgene, carbon monoxide, and chlorine are...
c) The standard enthalpies of formation and molar entropies of phosgene, carbon monoxide, and chlorine are COCl2(g): ΔfH° = -220.08 kJ mol-1; S° = 283.8 J mol-1 K-1 CO(g): ΔfH° = -110.53 kJ mol-1; S° = 197.66 J mol-1 K-1 Cl2(g): ΔfH° = 0 kJ mol-1; S° = 223.08 J mol-1 K-1 i) Determine the reaction Gibbs energy for the decomposition of phosgene at 298 K. Is this reaction spontaneous at this temperature? [25 marks] ii) At what temperature does...
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) +...
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) + H2(g) + C2H6(g) ΔΗ° Substance (kJ/mol) C₂H4 52.4 C2H6 -84.68 0 -32.3 kJ -4.3 x 103 kJ 32.3 kJ 0 -137.1 kJ
8. From standard enthalpies of formation, standard entropies, and standard heat capacities available from tables in...
8. From standard enthalpies of formation, standard entropies, and standard heat capacities available from tables in the Data section (pp 572-579), calculate the standard enthalpies and entropies at 298 K and 398 K for the reaction CO2(g)+ H2(g) -> CO(g) + H20(g). Assume that the heat capacities are constant over the temperature range involved. Recall that the standard reaction enthalpy and entropy are given by Products Reactants 0 7n 0 Products Reactants List the fundamental concepts involved in this problem.]
10. Using the table of standard formation enthalpies that you will find below, calculate the reaction...
10. Using the table of standard formation enthalpies that you will find below, calculate the reaction enthalpy of this reaction under standard conditions: 8H2S(g)+ 402(g) Ss(s) + 8H2O(0) Round your answer to the nearest kJ. reactant or product H2S(g Ss(s) Standard formation rection -206 H(+ 8SH2Sg) 0 0 H2O)
Calculate the standard enthalpy of formation of gaseous sulfur dioxide (S02) using the following thermochemical information: 2 Mgo(s) = 2 Mg(s) + O2(g) Mg(s) + S(s) = MgS(s) Mgs(s) + 2 Mgo(s) = 3 Mg(s) + SO2(g) AH = +1203.4 k) AH = -598.0 kJ AH = +1504.6 kJ AH = k]
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous carbon dioxide and liquid water at 25 °c (AHe AH/kJ mol 393.5 -285.9 -1559.7 C(graphite) H2(g) C2Ho(g) 5.9 131.0 229.5 Calculate the enthalpy change (AH) and Gibbs energy change (AG) for the reaction 2C(graphite) +3H28)CH) datseatt Is this reaction thermodynamically possible? Give a reason for your answer. (10 marks) Explain why it is possible for endothermic processes to occur spontaneously. 15 marks]
Calculate [delta H0 f] in kJ for the equation below using the
standard enthalpies of formation seen in the image:
Testbank, Question 6.123 Using the standard enthalpies of formation, AH : CO(g) = -110.5 kJ mol-1 CO2(g) = -393.5 kJ molt SO2(g) = -296.9 kJ molt SO3(g) = -395.2 k) mol-1 calculate AH reaction for CO2(g) + SO2(g) — 503(9) + CO(g)
10. (10 points) Use standard enthalpies of formation listed in the attached table to find AH° values for the following reaction at 25°C. NH3(g) + HCl(g) + NH4Cl (s) Substance NH3(g) HCl(g) NHACI (s) AH f (kJ/mol) -45.9 -92.31 -314.43 Is the reaction endothermic or exothermic?
for the following rxn Use the standard enthalpies of formation to calculate AH° reaction. C2H4(g) + H2(g) + C2H6(g) ΔΗ° Substance (kJ/mol) C₂H4 52.4 C2H6 -84.68 0 -32.3 kJ -4.3 x 103 kJ 32.3 kJ 0 -137.1 kJ
8. From standard enthalpies of formation, standard entropies, and standard heat capacities available from tables in the Data section (pp 572-579), calculate the standard enthalpies and entropies at 298 K and 398 K for the reaction CO2(g)+ H2(g) -> CO(g) + H20(g). Assume that the heat capacities are constant over the temperature range involved. Recall that the standard reaction enthalpy and entropy are given by Products Reactants 0 7n 0 Products Reactants List the fundamental concepts involved in this problem.]
10. Using the table of standard formation enthalpies that you will find below, calculate the reaction enthalpy of this reaction under standard conditions: 8H2S(g)+ 402(g) Ss(s) + 8H2O(0) Round your answer to the nearest kJ. reactant or product H2S(g Ss(s) Standard formation rection -206 H(+ 8SH2Sg) 0 0 H2O)
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