Calorimetry and Energy Balance

For the formula:
 Q= m c ∆T
The  units for specific heat are:

• g /J °C
• °C/g J
• kJ/g
• J/g°C

Tags

NGSS.HS-PS3-4

What would be the effect on the particles if more heat is supplied to the system?

• They would slow down
• They would stop moving
• They would speed up
• There would be no effect

Tags

NGSS.HS-PS1-5

NGSS.HS-PS3-2

If two objects have different temperatures, heat will flow from the warmer object to the cooler one UNTIL ____________

• one reaches a temperature of zero
• they both have an equal temperature
• one runs out of energy

Tags

NGSS.HS-PS3-4

The total energy of all the particles in a substance is called: 

• temperature
• thermal energy
• degrees
• mass

Tags

NGSS.HS-PS3-4

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C?  (show your work)

• -80,256
• 80.256
• 80,256
• -80.256

Tags

NGSS.HS-PS3-4

What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water?  The water weighs 75. g and had an initial temperature of 20.00 °C.
(Specific heat of water is 4.18 J/g°C).

• 0.111 J/g°C
• 1.29 J/g°C
• 0.129 J/g°C
• 22225.85 J

Tags

NGSS.HS-PS3-4

For a skillet, used for cooking, do you want a high or low specific heat?

• High, so that it will need more energy to heat up
• Low, so that it will change temperature quickly

Tags

NGSS.HS-PS3-4

The SI unit of heat and energy is the __________.

• calorie
• heat
• joule
• watt

A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?  (show your work)

• 25g
• 30g
• 20g
• 50g

Tags

NGSS.HS-PS3-1

A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. Is the reaction endothermic or exothermic?

• Exothermic
• Endothermic

Tags

NGSS.HS-PS3-4