Using Hess’s Law to Calculate ΔH
Calculate ΔH for 2 NO(g) + O2(g) → N2O4(g) using the following information:
N2O4(g)2 NO(g) + O2(g)→→2 NO2(g)2 NO2(g)ΔHΔH==+57.9 kJ−114.1 kJ
Calculate for using the following information: Select one
| 2.7 kJ | |
| -55.2 kJ | |
| -85.5 kJ | |
| -171.0 kJ | |
| +55.2 kJ |
Using Hess’s Law to Calculate ΔH Calculate ΔH for 2 NO(g) + O2(g) → N2O4(g) using...
Applying Hess’s Law, from the enthalpies of reactions, 2NaCl(s) + H2O(l) --> 2HCl(g) + Na2O(s) ΔH = + 507.31 kJ NO(g) + NO2(g) + Na2O(s) --> 2NaNO2(s) ΔH = − 427.14 kJ NO(g) + NO2(g) --> N2O(g) + O2(g) ΔH = − 42.68 kJ 2HNO2(l) --> N2O(g) + O2(g) + H2O(l) ΔH = + 34.35 kJ Calculate the enthalpy change (ΔHrxn) for the reaction: HCl(g) + NaNO2(s) --> HNO2(l) + NaCl(s) (You should show work to get credit) 5-Magnesium burns...
Use Hess’s law to calculate ∆H° for the reaction:C(s) + 2H2(g) + ½O2(g) → CH3OH(l) ∆H°∘= ?using only the following data:H2(g) + ½O2(g) → H2O(l) ∆H°= -285.8 kJC(s) + O2(g) → CO2(g) ∆H°= -393.5 kJ2CH3OH(g) + 3O2(g) → 2CO2(g) + 4H2O(l) ∆H°= -1452.8 kJ
Hess’s Law (a) Calculate the ∆H for the reaction: CCl4(g) → C(s, graphite) + 2Cl2(g) using the following chemical equations and their respective enthalpy changes: C(s, graphite) + 2F2(g) → CF4(g) ∆H = -679.9 kJ CF4(g) + 2Cl2(g) → CCl4(g) + 2F2(g) ∆H = 573.2 kJ (b) Calculate the ∆H for the reaction: C(s, graphite) + 2H2O(g) → CH4(g) + O2(g) using the following chemical equations and their respective enthalpy changes: C(s, graphite) + O2(g) → CO2(g) ∆H = -394...
Calculate ΔH for the reaction: NO (g) + O (g) → NO2 (g) given the following information: NO(g) + O3(g) → NO2(g) + O2(g) ΔH = -198.9 kJ O3(g) → 3/2 O2(g) ΔH = -142.3 kJ O2(g) → 2 O(g) ΔH = 495.0 kJ I understand the basic concept for the problem, the 1/3 O2 is throwing me off. Thanks!
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 reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K. ______ kJ (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.45 atm and 1.55 atm, respectively. _____ kJ
Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g): 2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -198 kJ ΔH°f (kJ/mol) SO2(g) -297
Calculate the enthalpy of the reaction: 2 NO(g) + O2(g) --> 2 NO2(g) given the following reactions and enthalpies of formation: 1/2 N2(g) + O2(g) → NO2(g), ΔH = 33.2 kJ 1/2 N2(g) + 1/2 O2(g) → NO(g), ΔH = 90.2 kJ
2. Use Hess’s Law to determine the enthalpy of the reaction below. 2F2(g) + 2H2O(l) → 4HF(aq) + O2(g) DH˚= ? H2(g) + F2(g) → 2HF(aq) DH˚ = -546.6 kJ 2H2 (g) + O2(g) → 2H2O(l) DH˚ = -571.6 kJ a. 42 kJ b. -1120 kJ c. -251 kJ d. -521 kJ e. -1690 kJ
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