Calculate the standard enthalpy for the reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), given the following data: N2(g) + O2(g) → 2NO(g) ΔHrxn = -43.1 kcal mol-1   N2(g) + 3H2(g) → 2NH3(g) ΔHrxn = -21.9 kcal mol-1   2H2(g) + O2(g) → 2H2O(g) ΔHrxn = -115.6 kcal mol-1   Round your answer to 2 decimal places.

For the molecule shown below, provide the names for all of the indicated functional groups: O 3 1 aspirin 1. Functional group 1: 2. Functional group 2: 3. Functional group 3: 2 OH;

Given the standard enthalpy changes for the following two reactions: (1) 2Pb(s) + O₂(g) → 2PbO(s) ΔΗ° (2) Pb(s) + Cl₂(g) → PbCl₂ (s) ΔΗ° ΔΗ° what is the standard enthalpy change for the reaction: (3) 2PbCl₂ (s) + O2 (g) → 2PbO(s) + 2Cl₂(g) ΔΗ° =? = = 434.6 kJ - 359.4 kJ KJ =

Pentane (C5H12)(C5H12) is a component of gasoline that burns according to the following balanced equation:C5H12(l)+8O2(g)→5CO2(g)+6H2O(g) Calculate ΔH∘rxnΔHrxn∘ for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of liquid pentane is -146.8 kJ/molkJ/mol.)

Using standard heats of formation, calculate the standard enthalpy change for the following reaction. ΔΗ° rxn 4NH3(g) +502 (g) → 4NO(g) + 6H₂O(g) AH (NH3 (9)) = -46.1 kJ/mol AH (O₂ (g)) = 0.0 kJ/mol AH (NO(g)) = 90.3 kJ/mol AH (H₂O(g)) = -241.8 kJ/mol = KJ

If reacting 3.08 g of chlorine monoxide (ClO), a highly reactive radical, with an excess of ozone (O3) produces 1.65 kcal of heat, then what is the enthalpy change for the following reaction (in kcal/mol)?  ClO (g) + O3 (g) → Cl (g) + 2 O2 (g)

A scientist measures the standard enthalpy change for the following reaction to be 215.5 kJ : CH4(g) + H20(g)→3H2(g) + CO(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H,O(g) is kJ/mol.

Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product smells vile. Carbon disulfide is used in the manufacture of rayon and cellophane. The liquid burns as follows: CS2(ℓ) + 3O2(g) → CO2(g) + 2SO2(g) Calculate the standard enthalpy change for this reaction using standard enthalpies of formation. ΔH°f (CS2(ℓ)) = 89.70 kJ ΔH°f (CO2(g)) = -393.52 kJ ΔH°f (SO2(g)) = -296.8 kJ

Using the Table of Thermodynamic Values, determine the change in enthalpy (kJ) for the following reaction.  Use all significant figures provided in the Table of Thermodynamic Values.  Do not type units into your answer.   2 NaOH(s) + 2 HCl(aq) ⟶⟶ 2 H2O(l) + 2 NaCl(aq)     Δ?=?ΔH=?

At constant volume, the heat of combustion of a particular compound, compound A, is −3520.0 kJ/mol.−3520.0 kJ/mol. When 1.439 g1.439 g of compound A (molar mass =112.71 g/mol)=112.71 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.391 ∘C.6.391 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?