Calorimetry

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

• g /J C
• °C/g J
• kJ/g
• J/g°C

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

Thermal energy ALWAYS moves from _____ to _____.

• solid to liquid
• ice to water
• hot to cold
• solid to gas

LT3: 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 movement of thermal energy from an object at a higher temperature to an object at a lower temperature is called ____________.

• thermal
• expansion
• temperature
• heat

Tags

NGSS.MS-PS1-4

NGSS.MS-PS3-4

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

• temperature
• thermal energy
• degrees
• mass

If the specific heat of water is 4,186 J/kg∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? 

• -80,371.2
• 44,938.6
• 80,371.2
• 112,575.9

What is the specific heat of an unknown substance if 20 kg of it at 400 °C reaches an equilibrium temperature of 351 °C when it comes in contact with a piece of aluminum.  The aluminum weighs 55 kg and had an initial temperature of 4 °C?  (Specific heat of aluminum is 903 J/kg °C)  Use the equation mC(T_f – T_i) + mC(T_f – T_i)= 0

• 17,233,755
• -17,233,755
• 17,585.46
• 723

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

Steam at temperature of 100°C is piped to 3 kg of water at the temperature of 5°C until the water reaches the boiling point. The mass of the steam required is
[Specific latent heat of vaporization of water = 2.26 × 10⁶ J kg⁻¹, specific heat capacity of water = 4.2 × 10³ J kg⁻¹°C⁻¹]

• 0.26 kg
• 0.53 kg
• 0.94 kg
• 1.89 kg

How many Joules of energy are required to make 100 grams of ice at 0 ^οC completely melt?

• 200 J
• 400 J
• 30,000 J
• 2,000,000 J