Write the net ionic equations for each of the reactions and give the molar entha

Question

Write the net ionic equations for each of the reactions and give the molar enthalpy for each reaction. Predict the value of the expected molar enthalpy for the reaction 3 from the molar enthalpies for reactions 1 and 2. As a test of the validity of Hess's Law, compare the calculated and experimental values by reporting the percent relative difference for these values: I conducted this experiment in lab so if you need any other calculations that I got from the experiment, let me know. Reaction 1 NaOH (aq) + HCl (aq) --> H2O (l) + NaCl (aq) 1.0M 1.0M Reaction 2 NaOH (s) ---> NaOh (aq) 1.0M Reaction 3 NaOH (s) + HCl (aq) ---> H20 (l) + NaCl (aq) 1.0M %Relative Difference = -absolute value of [(deltaH of reaction 3 - deltaH of reaction 2 and 3)/ deltaH of reaction 3] X 100%

Explanation / Answer

1)Chemical Reaction: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)

Heat of formation:.....-469.15 .... -92.30 ...... -407.27 ... -285.83 ... all in kJ/mol

Hess's Law: ΔH(rxn) = Sum[ΔH(f) products] - Sum[ΔH(f) reactants]

ΔH(rxn) = [(1 mol)(-407.27 kJ/mol) + (1 mol)(-285.83 kJ/mol)] - [(1 mol)(-469.15 kJ/mol) + (1 mol)(-92.30)]

ΔH(rxn)=-131.65kJ/mol

see here i have used some values stand.as you have given none so if there is any other value in book just simply put it and get its just maths.

H+ (aq) + Cl- (aq) + Na+ (aq) + OH- (aq) --> H2O (l) + Na+ (aq) + Cl- (aq)

The net ionic eqn is the same as the total, or complete, ionic equation except that the spectator ions are left out. Spectator ions are those that appear on both the product side and the reactant side.

H+ (aq) + OH- (aq) --> H2O (l)

2)NaOH (s) ---> NaOH (aq)

The ∆H is -425.93kJ/Mol

3)NaOH (s) + HCl (aq) ---> H20 (l) + NaCl (aq)

adding 1) and 2) we get the final rxn so

∆H=-425.93-131.65=-557.58kJ/mol

Relative Difference = -absolute value of [(deltaH of reaction 3 - deltaH of reaction 2 and 3)/ deltaH of reaction 3] X 100%

ALL THE values are given just put in formula and get the final result

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