Assuming that the specific heat of the solution is 4.18 j/(g⋅∘c), that its density is 1.00 g/ml, and that the calorimeter itself absorbs a negligible amount of heat, calculate δh in kilojoules for the reaction. h2so4(aq)+2naoh→2h2o(l)+na2so4(aq)
Answer:
Q= mcâ†T
Q = energy (heat) generated or absorbed
m = mass of the substance undergoing the change in temperature
c = specific heat of the substance undergoing the change in temperature
â†T = T(final) - T(initial)
We are given:
m = (25.0 mL + 50.0 mL)*(1.00 g/mL) = 75.0 g
c = 4.18 J g^-1 °C^-1
â†T = 33.9 °C - 25.0 °C = 8.9 °C
Now we just plug those numbers in:
Q= mcâ†T
Q = (75.0 g)*(4.18 J g^-1 °C^-1)*(8.9 °C)
Q = 2790.15 J = 2.79 kJ (to three sig figs)
