The addition of hydrochloric acid to a silver nitrate solution precipitates silv

Question

The addition of hydrochloric acid to a silver nitrate solution precipitates silver chloride according to the reaction: AgNO_3(aq) + HCl(aq) rightarrow AgCl(s) + HNO_3(aq) When you combine 80.0 mL of 0.110 M AgNO_3 with 80.0 mL of 0.110 M HCl in a coffee-cup calorimeter, the temperature changes from 23.25 degree C to 24.35 degree C. Calculate delta H_rxn for the reaction as written. Use 1.00 g/mL as the density of the solution and C = 4.18 J/g middot degree C as the specific heat capacity. Express your answer with the appropriate units.

Explanation / Answer

(4.18 J/g°C) x ((80.0 mL + 80.0 mL) x (1.00 g/mL)) x (24.35 - 23.25) °C = 735.68 J

There is no excess and either could be considered the limiting reactant, because The volume and concentration of both reactants are the same,

(0.0900 L) x (0.110 mol/L) = 9.9*10^-3mol each of AgNO3 and HCl

(1 mol AgNO3) x (735.68 J / 9.9*10^-3 mol) = 74311.11 J = 74.31 kJ

AgNO3(aq) + HCl(aq) AgCl(s) + HNO3(aq), H = - 74.31 kJ
[The minus sign which is present does not come from the calculations. It is the convention for exothermic processes.]

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