Question

During an experiment, a student adds 0.339 g of calcium metal to 100.0 mL of 2.05 M HCl. The student observes a temperature increase of 11.0 °C for the solution. Assuming the solution's final volume is 100.0 mL , the density is 1.00 g/mL , and the specific heat is 4.184 J/(g⋅°C) , calculate the heat of the reaction, ΔHrxn . Ca(s) 2H (aq)⟶Ca2 (aq) H2(g)

Answer 1

Answer:

The heat of the reaction is 17.94 J.

Explanation:

mass of Ca (m) = 0.339 g

increase in temperature (∆T)= 11°C

specific heat (s)= 4.184 J/(g. °C)

Now, to calculate the total heat we will have to multiply the mass with specific heat and increase in temperature.

∆H = m × s × ∆T

      = 0.339 × 4.184 × 11

      = 17.94 J