Zinc metal reacts with hydrochloric acid according to this balanced equation. zn(s) 2hcl(aq)→zncl2(aq) h2(g) when 0.114 g of zn(s) is combined with enough hcl to make 52.4 ml of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.0 ∘c to 23.9 ∘c.

The enthalpy change of the reaction is 239.2 kJ/mol

Explanation:

Density of solution = 1.0 g/mL

Volume of solution = 52.4 mL

Putting values in above equation, we get:

where,

q = heat absorbed = ?

m = mass of solution = 52.4 g

c = specific heat capacity of solution = 4.18 J/g.°C

= change in temperature =

Putting values in above equation, we get:

Heat absorbed by the solution = heat released by the reaction

Given mass of zinc = 0.114 g

Molar mass of zinc = 65.4 g/mol

Putting values in above equation, we get:

Conversion factor:  1 kJ = 1000 J

Hence, the enthalpy change of the reaction is 239.2 kJ/mol

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