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The addition of hydrochloric acid to a silver nitrate solution precipitates silver chloride according to the reaction:
AgNO3(aq)+HCl(aq)→AgCl(s)+HNO3(aq)
When you combine 70.0mL of 0.185M AgNO3 with 70.0mL of 0.185M HCl in a coffee-cup calorimeter, the temperature changes from 23.16∘C to 24.25∘C.
Calculate ΔHrxn for the reaction as written. Use 1.00 g/mL as the density of the solution and C=4.18J/g⋅∘C as the specific heat capacity.,
Δ H reaction = q / n where q: amount of heat released and n is number of moles of substance. q = m . C . ΔT where: m = mass of substance (g) C = Specific heat capacity (4.18) ΔT = change in temperature = 24.25 - 23.16 = 1.09 q = 1000 x 4.18 x 1.09 = 4556 J = 4.556 kJ number of moles (n) = Molarity (M) x Volume (L) = 0.185 M x 0.07 L = 0.01295 mole Δ H = q / n = - (4.556 kJ / 0.01295 mole) = -351.8 kJ / mol Note: it is exothermic reaction (-ve sign) i.e. temperature is raised
