Question

1. You will investigate three reactions in this experiment. In thespace provided below, write the balanced molecular and net ionicequations from the descriptions of the reactions. Use the table ofstandard heats of formation in your text (or another approvedresource) to calculate the molar enthalpies of the reactions.

• Reaction 1: An aqueous solution of sodium hydroxide reacts withan aqueous solution of hydrochloric acid, yielding water.

• Reaction 2: An aqueous solution of sodium hydroxide reacts withan aqueous solution of ammonium chloride, yielding aqueous ammonia,NH3, and water.

• Reaction 3: An aqueous solution of hydrochloric acid reacts withaqueous ammonia, NH3, yielding aqueous ammonium chloride.

Reaction	Balanced Reaction Equation	?H (KJ)
1	NaOH(aq) + HCl(aq) -> NaCl(aq) + H2O(l) Net ionic: H+ (aq) + OH- (aq) -> H2O (l)
2	NaOH(aq) + NH4Cl(aq) -> NaCl(aq) + NH3(g) + H2O(l) Net ionic: NH4+ (aq) + OH- (aq) -> NH3(g) + H2O(l)
3	HCl(aq) + NH3(aq) -> NH4+ + Cl- Net ionic: H+ (aq) + NH3 (aq) -> NH4+

1. For each reaction you perform, you will mix together 50.0 mL of2.00 M acid and 2.00 M base. What are the resulting concentrationsof the reactants upon mixing?
2. How many moles of each reactant are present in each trial?
3. What is the total volume of the solutions upon mixing? Assuminga density of 1.03 g/mL for the solution, find the total mass ofeach reaction mixture.

Hello, I have what I think are the right balanced equations butI can't figure out how to calculate the enthalpy (delta H) and I'munsure of how to do questions 1, 2, and 3 after the table.