how would i calculate the heat produced by this reaction?

Question

When 25.0 mL of 1.5 M H₂SO₄ (aq) and 50.0 mL of 2.0 M NaOH(aq), both at 25.0 °C are added to a coffee cup calorimeter, the temperature of the mixture reaches a maximum of 28.9 °C. What is the approximate amount of heat produced by this reaction? (𝐶𝑠 𝑜𝑓 𝑤𝑎𝑡𝑒𝑟 = 4.184 J/g ∘C) Assume the density of all solutions to be 1.0 g/mL.

equation given: H₂SO₄ + 2 NaOH → Na₂SO₄ + 2 H₂O

Answer 1

H₂SO₄ + 2 NaOH → Na₂SO₄ + 2 H₂O

To calculate the heat produced by the reaction, use q = mC∆T

q = heat

m = mass of the solution = 25.0 ml + 50.0 ml = 75.0 ml x 1 g / ml = 75.0 g of solution

C = specific heat = 4.184 J/gº

∆T = change in temperature = 28.9º - 25.0º = 3.90º

q = (75.0 g)(4.184 J/gº)(3.9º)

q = 1223.8 J = 1220 J (3 sig. figs.)

Note: the balanced reaction and the concentrations of H2SO4 and NaOH don't come into play unless you wanted to find the ∆Hrxn of reaction on a per mole basis.