Quiz Review: Heat

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1,200 g of water from 23 °C to 39 °C?

• -80,256 J

• 80.256 J

• 80,256 J

• -80.256 J

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

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?

• 25g

• 30g

• 20g

• 50g

Tags

NGSS.HS-PS3-4

What is the formula to calculate heat energy required to raise the temperature of any substance?

• Q = m C ∆T

• Q = m Hv

• Q = ½ m v

• m = Q Hf

In heat capacity equations, what does the triangle represent?

• Temperature

• energy

• mass

• change in

• change in temp

How many Joules of energy are required to make 50.0 grams of ice at 0 ^οC completely melt?

• 334 J

• 0 J

• 33,400 J

• 16,700 J

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-2

The temperature of a 6.0 g sample of glass changed from 20.0°C to 45.0°C when it absorbed 550 J of heat. What is the specific heat of this glass?

• 0.27 J/g °C

• 3.7 J/g °C

• 130 J/g °C

• 12 J/g °C

Tags

NGSS.HS-PS3-1

Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using 10,000 JOULES of thermal energy.  What material would be have the LARGEST change in temperature?

• Copper
• Carbon Steel
• Zinc
• Stainless Steel

Tags

NGSS.HS-PS3-4

For an exothermic reaction, the heat is on the ____ side

• reactant
• product
• either side

For an endothermic reaction, the heat is on the ____ side.

• reactant
• product
• either side

Tags

NGSS.HS-PS1-4

Exothermic reaction:

• delta H is positive
• delta H is negative
• delta H is zero

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1