Consider the following data.
2 H2(g) + O2(g) 2 H2O(l) ΔH = -571.7 kJ
N2O5(g) + H2O(l) 2 HNO3(l) ΔH = -92.0 kJ
N2(g) + 3 O2(g) + H2(g) 2 HNO3O(l) ΔH = -348.2 kJ
Use Hess's law to calculate ΔH for the reaction below.
2 N2O5(g) 2 N2(g) + 5 O2(g)
ΔH = _____kJ
Consider the following data. 2 H2(g) + O2(g) 2 H2O(l) ΔH = -571.7 kJ N2O5(g) +...
5. Given the following data: (2 H2 (g) + O2 (g) → 2 H2O (1) ro in each AH° = -571.6 kJ N20s (g) + H2O (1) 2 HNO3 (1) AH° = -76.6 kJ N2 (g) + 3 O2 (g) + H2 (g) → 2 HNO3 (1) AH° = -348.2 kJ a. Calculate the AHⓇ for the reaction: 2 N2 (g) + 5 O2 (g) → 2 N2O5 (g)
Consider the following data. CH4(g) C(s) + 2 H2(g) H = +74.8 kJ C(s) + O2(g) CO2(g) H = -393.5 kJ 2 H2(g) + O2(g) 2 H2O(l) H = -571.7 kJ Use Hess's law to calculate H for the reaction below. CH4(g) + 2 O2(g) CO2(g) + 2 H2O(l) H = _____ kJ
Consider the following data. 2 C(s) + H2(g) C2H2(g) H = +226.8 kJ CO2(g) C(s) + O2(g) H = +393.5 kJ 2 H2O(l) 2 H2(g) + O2(g) H = +571.7 kJ Use Hess's law to calculate H for the reaction below. 2 C2H2(g) + 5 O2(g) 4 CO2(g) + 2 H2O(l) find kJ
Calculate the standard enthalpy of formation of liquid water (H2O) using the following thermochemical information: 2 HNO3(l) N2O5(g) + H2O(l) H = +92.0 kJ 2 N2(g) + 5 O2(g) 2 N2O5(g) H = +59.3 kJ N2(g) + 3 O2(g) + H2(g) 2 HNO3(l) H = -348.2 kJ
2. Given the following data: H2O(l) → H2(g) + 1/2O2(g) ΔH° = 285.8 kJ 2HNO3(l) → N2O5(g) + H2O(l) ΔH° = 76.6 kJ 2N2(g) + 5O2(g) → 2N2O5(g) ΔH° = 28.4 kJ Calculate ΔH° for the reaction: 1/2N2(g) + 3/2O2(g) + 1/2H2(g) → HNO3(l) Note that you should be able to answer this one without needing to use any additional information from the thermo table. I've attempted this question multiple times. I am able to get to the simplified eqaution...
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
Using the reactions below, determine the ∆Hº for 2 N2(g) + 5 O2(g) --> 2 N2O5(g) N2(g) + 3 O2(g) + H2(g) --> 2 HNO3(aq) ∆Hº = -415 kJ/mol N2O5(g) + H2O(l) --> 2 HNO3(aq) ∆Hº = -140 kJ/mol 2 H2(g) + O2(g) --> 2 H2O(l) ∆Hº = -572 kJ/mol
Given the following equations and Ho values given below, determine the heat of reaction at 298 K for the reaction: 2 N2(g) + 5 O2(g) 2 N2O5(g) 2 H2(g) + O2(g) 2 H2O(l) Ho/kJ = -571.6 N2O5(g) + H2O(l) 2 HNO3(l) Ho/kJ = -73.7 N2(g) + 3 O2(g) + H2(g) 2 HNO3(l) Ho/kJ = -348.2
Consider the reaction: H2(g) + (1/2)O2(g) -------> H2O(l) ΔH° = -286 kJ Which of the following is true? (Select all that apply) the reaction is endothermic heat is given off by the surroundings the reaction is exothermic heat is absorbed by the system the enthalpy of the products is less than the that of the reactants
Consider the following data. 2 NO(g) N2(g) + O2(g) H = -180.7 kJ 2 NO(g) + O2(g) 2 NO2(g) H = -113.1 kJ 2 N2O(g) 2 N2(g) + O2(g) H = -163.2 kJ Use Hess's law to calculate H for the reaction below. N2O(g) + NO2(g) 3 NO(g) H =_______ kJ