Answer:
1. To find the mass of water inside the calorimeter, subtract the mass of the calorimeter from the mass of the calorimeter and water.
Trial 1: 2.7691g - 1.3470g = 1.4221g
Trial 2: 2.4351g - 1.3210g = 1.1141g
2. To find the temperature change of the copper, subtract the initial temperature from the highest temperature reached.
Trial 1: 29.6°C - 22.4°C = 7.2°C
Trial 2: 29.8°C - 22.6°C = 7.2°C
3. To find the temperature change of the water inside the calorimeter, subtract the initial temperature from the highest temperature reached.
Trial 1: 29.6°C - 22.4°C = 7.2°C
Trial 2: 29.8°C - 22.6°C = 7.2°C
4. To find the specific heat capacity of copper, use the formula q = mcΔT, where q is the heat absorbed by the copper, m is the mass of the copper, c is the specific heat capacity of copper, and ΔT is the temperature change of the copper.
Trial 1: q = mcΔT = (1.5990g)(0.385J/g°C)(7.2°C) = 4.32J
c = q/mΔT = 4.32J/(1.5990g)(7.2°C) = 0.356J/g°C
Trial 2: q = mcΔT = (1.6193g)(0.385J/g°C)(7.2°C) = 4.37J
c = q/mΔT = 4.37J/(1.6193g)(7.2°C) = 0.361J/g°C
5. To find the average specific heat capacity of copper, add the specific heat capacity of copper for trial 1 to the specific heat capacity of copper for trial 2 and divide by 2.
Average: (0.356J/g°C + 0.361J/g°C)/2 = 0.358J/g°C