The standard enthalpy of formation of gaseous nitrogen dioxide is 33.2 kJ/mol, liquid water is -285.8 kJ/mol, aqueous nitric acid is -207 kJ/mol and the standard enthalpy of formation of gaseous nitrogen monoxide is 91.3 kJ/mol . Calculate the ΔHorxn for the following reaction:   3NO2(g) +  H2O(l)   →   2 HNO3(aq) + NO(g)

Nitric oxide (NO) can be formed from nitrogen, hydrogen and oxygen in two steps. In the first step, nitrogen and hydrogen react to form ammonia:N2(g) + 3H2(g) → 2NH3(g) =ΔH−92.kJIn the second step, ammonia and oxygen react to form nitric oxide and water:4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) =ΔH−905.kJCalculate the net change in enthalpy for the formation of one mole of nitric oxide from nitrogen, hydrogen and oxygen from these reactions.Round your answer to the nearest kJ.

The enthalpy of formation of NH3 is – 46. The enthalpy change for the reaction: 2NH3 → N2 + 3H2 is ?46 KJ92 KJ–23 KJ     –92 KJ

Calculate ΔrG(in kJ/mol) for given reaction at 300 KN2(g) + O2(g) ⇌ 2NO(g)the partial pressure of N2, O2 & NO are 10–4 bar, 10–2 bar and 10–5 bar respectively when mixed together at 300 K.Given : 2.303 RT = 5750 J/molAt 300 K standard enthalpy of formation of NO(g) = 90.5 kJ mol–1,Standard molar entropy data at 300 K :S°(N2, g) = 190 J K–1 mol–1S°(NO, g) = 210 J K–1 mol–1S°(O2,g) = 205 J K–1 mol–1 ?

4. Consider the reaction:N2(g) + O2(g) → 2NO(g) ΔHo = 180.5 kJIf 124 kJ of heat is absorbed in a reaction that forms nitric oxide from nitrogen and oxygen, what mass of NO must have been produced? What mass of N2 was consumed?5. Using these reactions, find the standard enthalpy change for the formation of 1 mol PbO(s) from lead metal and oxygen gas. If250. g of lead reacts with oxygen to form lead(II) oxide, what quantity of thermal energy (in kJ) is absorbed or evolved?

The equilibrium constant for the reaction below is 7.2 × 10-4at 298 K and 1 atm.HNO2(aq) + H2O(l) NO2-(aq) + H3O+(aq)When [HNO2(aq)] = 1.0 M and [NO2-(aq)] = [H3O+(aq)] = 1.0× 10-5 M, calculate ΔG.