8 marks (a) Given the following information: AH = -116 kJ AH = -256 kJ Eqn. 1: Eqn. 2: 2NO(g) + O2(g) 2NO2(g) 2N2(g) + 502(g) + 2H2O(C) ► 4HNO3(aq) N2(g) + O2(g) → 2NO(g) AH = +183 kJ Eqn. 3: Use Hess's Law to calculate the enthalpy change for the reaction below (Show your working) AHrın = ??? 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) AHHO

Hess's law states that the enthalpy for the whole reaction will be equal to the summation of all changes that are independent of the steps of the reaction.

First, arrange all the reactions and balance them, first the data of equation 1 is rearranged:

NO₂ must be on the reactant side and must be multiplied by 3/2 so that 3 moles of NO are balanced.

3 NO₂ (g) → 3 NO (g) + 3/2 O₂ (g), ΔH = + 174 kJ

Now, for equation 2: the moles of HNO₃ required is 2 so the whole equation will be divided by 2 as,

N₂ (g) + 5/2 O₂ (g) + H₂O (l) → 2HNO₃ (aq), Δ H = -128 kJ

Now, for equation 3: N₂ and O₂ should be eliminated and reversed as,

2NO (g) → N₂(g) + O₂(g) ΔH = -183 kJ

Now, to determine the enthalpy the rearranged equation 1, 2, and 3 are added to get the final equation:

3NO₂ (g) + H₂O (l) → 2HNO₃ (aq) + NO (g)

Δ H = 174 - 128 - 183

= -137 kJ

Therefore, -137 kJ is the enthalpy change.

Learn more about Hess's law here:

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