CHM113 Prelab Quiz 5: Hot Water

In a calorimetry experiment, it was determined that the heat change of the surroundings, qsurroudings, was 4482 J. What is the heat change of the system, qsystem?

-4482 J

A 10.0 gram piece of metal is placed in an insulated calorimeter containing 250.0 grams of water initially at 20.0°C. If the final temperature of the mixture is 25.0°C, what is the heat change of piece of metal?

-5230 J

What is the specific heat of liquid water, written with correct units? Refer to Table 5.2 or Appendix B in your textbook, or your lecture notes.

4.184 J/(g C)

A 10.0 gram piece of metal is placed in an insulated calorimeter containing 250.0 g of water initially at 20.0°C. If the final temperature of the mixture is 25.0°C, what is the heat change of water?

5230 J

What can we say about the temperature change of a sample of water when the value of q is negative?

The temperature of the water decreased.

In a calorimetry experiment, it was determined that a 92.0 gram piece of copper metal released 1860 J of heat to the surrounding water in the calorimeter (qcopper = −1860 J). If the final temperature of the copper metal-water mixture was 25.00°C, what was the initial temperature of the copper metal? The specific heat of copper is 0.377 J/(g°C).

Tinitial = 78.6°C

True or False. Although chemicals aren't used in this investigation, glassware will be used, so PPE is required.

True

True or False. The thermometer used for this investigation only reaches a temperature of ~40 degrees celsius, so the objective is to mathematically determine the initial temperature of hot water. The picture below shows the set-up for the calorimeter apparatus that will be used for this investigation.

True

When the surroundings absorbs heat, is the heat change of the system (qsystem) positive or negative?

negative (<0)

When the surroundings absorbs heat, is the heat change (qsurroundings) positive or negative?

positive (>0)