Answer:
see explanation
Explanation:
Step 1: Data given
Volume of 1M CusO4 = 50.0 mL = 0.05 L
Volume of 2M KOH = 50.0 mL = 0.05 L
Temperature before mixing= 17.8 °C
Temperature after mixing = 32.4 °C
The heat capacity of the calorimeter is 12.1 J/K
Step 2: The balanced equation
CuSO4(aq)+ 2KOH(aq) →Cu(OH)2(s) + K2SO4(aq)
Step 3: Calculate mass of the solution
Suppose the density of the solution is 1 g/mL
Total volume = 100 mL
Mass of the solution = density * volume
Mass of the solution = 1g/mL * 100 mL = 100 grams
Step 4:
Q = m*c*ΔT
with m = the mass of the solution = 100 grams
with c= the heat capacity of the solution = 4.184 J/g°C
with ΔT = 32.4 - 17. 8 = 14.6 °C
Q = 6108.64 J
Step 5: Calculate the energy of the calorimeter
Q = c*ΔT
Q = 12.1 J/K * 14.6
Q = 176.66 J
Step 6: Calculate total heat
Qtotal = 6108.64 + 176.66 = 6285.3 J = 6.29 kJ (negative because it's exothermic)
Step 7: Calculate moles
Moles CuSO4 = 0.05 L * 1M = 0.05 moles
Moles KOH = 0.05 L * 2M = 0.10 moles
ΔH = -6.29 kJ / 0.05 moles = -125.8 kJ/mol
