Specific Heat Problems

A 15.75-g piece of iron absorbs 186.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron.

• 0.46 J/g^oC

• 1.65 J/g^oC

• 441196.88 J/g^oC

• .08 J/g^oC

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/gx°C?

• 297 Joules

• 0.003 Joules

• 297 J/gx°C

• 0.003 J/gx°C

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

A 0.3 g piece of copper is heated and fashioned into a bracelet. The amount of energy transferred by heat to the copper is 66,300 J. If the specific heat of copper is 390 J/g ⁰C, what Is the change of the copper's temperature?

• 566.67 °C

• 77,571,000 °C

• 647.33 °C

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

The temperature of a sample of water increases from 20°C to 46°C as it absorbs 5650 joules of heat. What is the mass of the sample? (Specific heat of water is 4.18 J/g°C.)

• 51.98 g

• 65.3 g

• 51.99 g

Tags

NGSS.MS-PS1-4

NGSS.MS-PS3-4

A 4.50 g coin of copper absorbed 254 Joules of heat. What was the change in temperature of the copper? The specific heat of copper is .385 J/g^oC.

• 210 ^oC

• 146.61 ^oC

• 244.8 ^oC

Tags

NGSS.HS-PS3-4

The specific heat of aluminum is 0.9 J/goC. If 5490 J of heat is added and the temperature changes from 2 ^oC to 92 ^oC, what is the mass of the aluminum?

• 278 g

• 67.78 g

• 444690 g

• 45.89 g

Tags

NGSS.HS-PS3-4

The specific heat of gold is .129 J/goC. If 918.69J is added to 47 grams of gold, what will be the resulting temperature change?

• 15.15 ^oC

• 478 ^oC

• 17 ^oC

• 151.52 ^oC

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4