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
The heat of the reaction at 298 K for the given reaction is +22.6 kJ .
The detail calculation is shown below .
Given the following equations and Ho values given below, determine the heat of reaction at 298...
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. 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
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
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
Part 1) Use the following equations to calculate the heat of the reaction for the formation of ethane (C2H6). C2H6(g) + 7/2 O2(g) → 2CO2(g) + 3 H2O(l) ∆ Ho = -1560 kJ C(gr) + O2(g) → CO2(g) ∆ Ho = -394 kJ H2(g) + 1/2 O2(g) → H2O(l) ∆ Ho = -286 kJ Calculate ∆Ho for the following reaction: 2 C(gr) + 3H2(g) → C2H6(g) ethane Use kJ for your answer. ΔHo = Part 2) Find the heat of...
5. Given the following data: 2 H2(g) + O2(g) → 2 H20 (1) AH° = -571.6 kJ N,Os (g) + H20 (1) ► 2 HNO (1) AH = -76.6 kJ N2(g) + 3 O2 (g) + H2(g) → 2 HNO, (1) AH = -348.2 kJ a. Calculate the AHⓇ for the reaction: 2 N2 (g) + 5 O2(g) → 2 N2Os (g)
From the following equations, calculate AH for the reaction 2N2(g) + + 5O2(g) → 2N2O5(g) AH = ? H2(g) + O2(9) H206) AH = -285.8 kJ N2O5(g) + H200 2HNO30 AH = -76.6 kJ N2(g) + 302(g) + H219) - 2HNO30) AH = -348.2 kJ
Given the following equations and AH' values: C(s) + O2(g) + CO2(g) AH = -393.5 kJ H2(g) + 1/2O2(g) - H20 (1) AH = -285.8 kJ 2C2H2 (8) + 5O2(g) + 4CO2(g) + 2H20 (1) AH'= -2598 kJ Determine the heat of reaction (in kJ) at 298 K for the reaction: 2C(s) + H2(8) C2H2 (8) 0-136.8 0-219.8 0-109.9 O-167.1 +226.2
1. From the following equations and enthalpies, determine the molar heat of formation of HNO2(aq) . NH4NO2(aq) → N2(g) + 2H2O(l) ∆H = -320.1 kJ NH3(aq) + HNO2(aq) → NH4NO2(aq) ∆H = -37.7 kJ 2NH3(aq) → N2(g) + 3H2(g) ∆H = +169.9 kJ H2(g) + 1/2 O2(g) → H2O(l) ∆H = -285.8 kJ
You are given the following data. AH = = -286.0 kJ H2(g) + 1/2O2(g) → H20(1) N2O5(9) + H20(1) → 2 HNO3(aq) 1/2 N2(9) + 3/2 02(9) + 1/2 H2(9) AH = -77.0 kJ HNO3(1) AH = -174.0 kJ Calculate the AH for the reaction given below. 2 N2(g) + 5 O2(g) → 2 N205(9) k] Need Help? Read It Supporting Materials Periodic Table E Constants & Factors Supplemental Data