Calorimetry part 5

Question

A 52.19 mL sample of 3.02 M CuSO4 reacts with 54.48 mL of 2.87 M KOH in a coffee cup calorimeter to form Cu(OH)2(s) and K2SO4 (aq). The initial temperature is 18.5°C and the final temperature is 44.9°C. Assume that the mixture has the same specific heat as water and the same density as water. Specific heat of water is 4.184 J/g-K.

e.) How much heat, in J, was transferred to the solution?

Answer 1

See previous answers...

q = mCΔT

w = heat = ?

m = mass = 52.19 ml + 54.48 ml = 106.67 ml = 106.67 g

C = specific heat = 4.184J/g/deg

ΔT = change in temperature = 44.9 - 18.5 = 26.4 deg

q = (106.67 g)(4.184 J/g/deg)(26.4 deg)

q = 11783 = 11,800 J