2 HNO3(aq) + NO(g) à 3 NO2(g) + H2O(l)
DHof (kJ/mol) -207 91.3 33.2 -285.8
So (J/mol . K) 146 210.8 240.1 70.0
Calculate the DGorxn using the following information. 2 HNO3(aq) + NO(g) à 3 NO2(g) + H2O(l)...
Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0 -151 kJ +50.8 kJ -186 kJ +222 kJ -85.5 kJ
Calculate the ΔG°rxn at 298 K using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0
1. Calculate ΔHnn for the following reaction. 3NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) Given. AHof (NO2(g)) = +33.2 klymol AHof (H20(1)) =-187.8 ki/mol AHof (HNO3(aq)) =-207.0 kJ/mol AHof (NO(g)) = +91.3 kJ/mol
Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1
Consider the following chemical reaction. NH3(g) + 2 O2(g) → HNO3(aq) + H2O(l) Calculate the change in enthalpy (ΔH) for this reaction, using Hess' law and the enthalpy changes for the reactions given below. (1a) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l); ΔH = −1166.0 kJ/mol (2a) 2 NO(g) + O2(g) → 2 NO2(g); ΔH = −116.2 kJ/mol (3a) 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g); ΔH = −137.3 kJ/mol
Consider the following reaction at 25 degree C: 2HNO_3 (aq) + NO(g) rlhar 3 NO_2(g) + H_2O(l) Calculate Delta G degree rxn using the following information HNO_3 (aq) NO(g) NO_2(g) H_2O(l) Delta H^degree (kJ/mol) -207 91.3 33.2 -285. 8 S^degree (J/mol K) 146 210.8 240.1 70.0 Calculate the value of the equilibrium constant, K, at 25 degree C At 25 degree C does the above reaction favor reactant or product formation? What evidence supports your conclusion? Procedure: Obtain the five...
Calculate ΔG°(in kJ/mol) for the reaction NO2(g) + H2O(l) --> HNO3(l) + NO(g). ( unbalanced) Substance ΔGfo(kJ/mol) NO2(g) 51.8 NO(g) 86.7 HNO3(l) -79.9 H2O(l) -237.2 Write answer to two significant figures and correct sign.
Calculate ΔG°(in kJ/mol) for the reaction NO2(g) +
H2O(l) --> HNO3(l) + NO(g).
(unbalanced)
Question 7 Calculate AG°(in kJ/mol) for the reaction NO2(g) + H2O(0) --> HNO3(1) + NO(g). (unbalanced) Substance AGF(kj/mol) NO2(g) 51.8 NO(g) 86.7 HNO3(0) -79.9 H2O(l) -237.2 Write answer to two significant figures and correct sign.
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
only worth 1 point. 1. (6) 15.0 g of ice cubes at 0.0°C are combined with 150.g of liquid water at 70.0°C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the calorimeter. (Data: specific heat capacity of H2O(l). C4.18 1/8 'C) H2O(s) → H2O(1) AH = 6.02 kJ/mol) 2. (6) Calculate A s for the reaction: 5C(s) + 6H2(g) → CsHuz10 Use the following reactions and given AH's. CsHua(l) + 802()...