Heat and Specific Heat

How much energy is required to heat up 12000 g of copper from 10 °C to 120 °C. The specific heat capacity is 0.390 J/g°C.

• 46800 J

• 561600 J

• 514800 J

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

The amount of energy required to raise the temperature 1ºC for every gram is called____?

• Thermal Energy

• Specific Heat

• Temperature

• Kinetic Energy

How much energy is needed to raise the temperature of 5.0 grams of lead from 25°C to 35°C? [specific heat (c) = 0.129 J/(g•°C)]

• 6.45 J/(g•°C)

• 6.45 J

• 16.1 J/(g•°C)

• d.16.1 J

Tags

NGSS.MS-PS3-4

NGSS.MS-PS3-5

The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?

• 12.82 °C

• 24.12°C

• 351 °C

Tags

NGSS.MS-PS1-4

NGSS.MS-PS3-4

Object A has a specific heat of 4.45 J/g⁰C and object B has a specific heat of 1.82 J/g⁰C. Which object will heat up faster?

• Object A, it has a lower specific heat

• Object B, it has a lower specific heat

• Object A, it has a higher specific heat

• Object B, it has a higher specific heat

The unit for specific heat is

• J

• J/gC

• g

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

• Q = m c ∆T

• Q = m c

• Q = ½ m v

• m = Q c

If the specific heat of water is 4.186 J/g∙°C, how much heat is required to increase the temperature of 1200g of water from 23 °C to 39 °C?

• -80,371.2 J

• 44,938.6 J

• 80,371.2 J

• -44,938.6 J

Tags

NGSS.MS-PS1-4

NGSS.MS-PS3-4

NGSS.MS-PS3-5

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.MS-PS1-4

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

• 25 g

• 30 g

• 20 g

• 50 g

Tags

NGSS.MS-PS3-4

NGSS.MS-PS3-5