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
Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 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
Calculate the AGºrxn using the following information. 2HNO3(aq) + NO(g) + 3NO2(g) + H20 (1) AG rxn = ? AG°f(kJ/mol)= -110.9 87.6 51.3 -237.1 O +162.5 kJ O +51.0 kJ O-74.9 kJ O +54.5 kJ -87.6 kJ
Calculate the DGorxn using the following information. 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
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:...
Calculate the LaTeX: \Delta Δ G°rxn using the following information. 4 HNO3(g) + 5 N2H4(l) LaTeX: \longrightarrow ⟶ 7 N2(g) + 12 H2O(l) LaTeX: \Delta Δ G°rxn = ? LaTeX: \Delta Δ G°f (kJ/mol) –73.5 149.3 –237.1
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.
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
9. Nitrogen dioxide (NO2) can react with water to form aqueous nitric acid according to the following reaction. This is one way that acid rain forms in the atmosphere. Also listed are the standard free energies of formation for the species involved in the reaction. 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) Compound AG, (kJ/mol) NO2(g) 51.3 H2O(0) -237.1 HNO3(aq) -110.9 NO(g) 87.6 a. Calculate AGºrx (6 points) b. Is the reaction spontaneous at standard conditions? Circle one and explain...