A calorimeter has a heat capacity of 50.0 J/°C. It contains 150.0 g of water. A reaction causes the temperature to rise from 22.0°C to 29.5°C. Calculate the total heat released.
If your answers match ours, you’re on track. If not, revisit your ΔT or moles calculation. calorimetry worksheet 2 answers chemsheets
Designed for A-level and high school chemistry students, this answer key does more than just provide final numbers—it guides you through the thermodynamic calculations needed to master heat transfer, specific heat capacity, and enthalpy change. A calorimeter has a heat capacity of 50
[ q = m \times c \times \Delta T ]
ΔH_combustion = -2230 kJ/mol (Literature value for ethanol is ~-1367 kJ/mol? Check – this high value indicates significant heat loss. In worksheet answers, they often accept calculated value; refine by using q = mcdT correctly. Actually recalc: 12.122 kJ / 0.005435 mol = 2230 kJ/mol. If heat loss ignored, it's correct per data.) Calculate the total heat released