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
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1. From the following equations and enthalpies, determine the molar heat of formation of HNO2(aq) ....
The formation of nitrous acid occurs as shown below: 202(g) + N2 (g) + H2(g) 2 HNO2 (aq) Apply Hess's law and calculate the AH (in kJ) for the above reaction. Useful thermochemical data are given below. Just type the final numerical answer with proper sign and sig figs. NH4NO2 (aq) -N2(g) + 2 H20 (1) NH3(aq) + HNO2 (aq) - NH4NO2 (aq) 2NH3(aq) + N2(g) + 3 H2(g) H2(g) + 1/2O2(g) + H20 (1) AH = - 320.1 kJ...
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(6 pts.) Using Hess’s Law and the values for Standard Enthalpies of Formation from the table provided, calculate the enthalpy of reaction ΔH°rxn (in kJ) for each of the following reactions: Standard Enthalpies of Formation substance ΔHf° in kJ/mol Mg(s) 0 MgO(s) -601.6 HCl(aq) -167.2 MgCl2(aq) -801.2 H2(g) 0 H2O(l) -285.8 Reaction #1: Mg (s) + 2HCl (aq) è MgCl2 (aq) + H2 (g) Reaction #2: MgO (s) + 2HCl (aq) è MgCl2 (aq) + H2O (l) 2. (4 pts.)...
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Standard Enthalpies of Formation, in kJ/mol N2(g) 0 NO2(g) +33.2 NH3(g) -45.9 H2O(l) -285.8 NO(g) +90.3 N2O(g) -82.1 H2O(g) -241.8 Use the data above to calculate ΔH for the reaction: 6 NO2(g) + 8 NH3(g) => 7 N2(g) + 12 H2O(g) ΔH = ?
3. You are given the following standard enthalpies of formation at 25°C. HF (aq) -320.1 kJ/mol OH(aq) -230.0 kJ/mol F (aq) -332.6 kJ/mol H:0 (1) -285.8 kJ/mol a. Calculate the standard enthalpy of neutralization of HF (aq) HF (aq) + OH(aq) F (aq) + H20 (1) b. Using the value of -56.2 kJ/mol as the standard enthalpy change for the reaction H' (aq) + OH(aq) - H20 (1) calculate the standard enthalpy change for the reaction HF (aq) - H(aq)...
A.Using standard heats of formation, calculate the standard enthalpy change for the following reaction. N2(g) + 3H2(g) = 2NH3(g) B.Using standard heats of formation, calculate the standard enthalpy change for the following reaction. CaCO3(s) = CaO(s) + CO2(g) C. A scientist measures the standard enthalpy change for the following reaction to be -2910.6 kJ: 2C2H6(g) + 7 O2(g) = 4CO2(g) + 6 H2O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy...
Using molar enthalpies of formation, determine the heat of reaction for the combustion of 1.0000 mole of methanol, 2CH3OHC) 30268) 2C02(8) 4H200 DHE kj/mol) -238.7 -393.5 -285.8 ca. -726.4 kJ b.-1452.8 kg C.-2407.6k d. -148.9K) e. -918.01