Heat Equations

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-PS3-4

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-PS3-1

NGSS.HS-PS3-4

The specific heat of water is 4.18 J/g°C.

If 980. J of energy is added to 6.20 g of water at 18.0 °C, what is the final temperature of the water?

• 37.8 °C

• -19.8 °C

• 19.8 °C

• 55.8 °C

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

How much heat is needed to change 12 grams of ice at 0 ºC to 12 grams of water at 0ºC?

• Q = 12 x 4.18 x 0

• Q = 12 x 334

• Q = 12000 x 334

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

The equation for calculating the energy involved in a substance being heated is Q = mCΔT. The correct expression for calculating ΔT is

• $=\frac{Q}{m\ \times C}$

• $=\ \frac{m\ \times C}{Q}$

• $=\ \frac{m\ \times Q}{C}$

• $=\ \frac{C\ \ \times\ Q}{m}$

Tags

NGSS.HS-PS3-4

In heat capacity equations, what does the triangle represent?

• Temperature

• energy

• mass

• change in

• change in temp

How much energy is required to raise 85.36 g of water from 18.5^oC to 60.3^oC?

• 21500 J

• 6610 J

• 14900 J

• 85400 J

Tags

NGSS.HS-PS3-1

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-PS3-4

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

NGSS.HS-PS3-4