Author Question: If a student performs an endothermic reaction in a calorimeter, how does the calculated value of H ... (Read 96 times)

audragclark · **on:** Mar 21, 2021

Question 1

If 5.0 kJ of energy is added to a 15.5-g sample of water at 10.°C, the water is:

◦ boiling.
◦ completely vaporized.
◦ frozen solid.
◦ decomposed.
◦ still a liquid.

Question 2

If a student performs an endothermic reaction in a calorimeter, how does the calculated value of ΔH differ from the actual value if the heat exchanged with the calorimeter is not taken into account?

◦ ΔH_calc would be more negative because the calorimeter always absorbs heat from the reaction.
◦ ΔH_calc would be less negative because the calorimeter would absorb heat from the reaction.
◦ ΔH_calc would be more positive because the reaction absorbs heat from the calorimeter.
◦ ΔH_calc would be less positive because the reaction absorbs heat from the calorimeter.
◦ ΔH_{_calc} would equal the actual value because the calorimeter does not absorb heat.

Jayson · **Reply #1 on:** Mar 21, 2021

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