Specific Heat Problems

20 g of water. specific heat of water is 4.18 J/x°C.  temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings?

• 418 Joules
• 209 J
• 83 J
• 4.18 J

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

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.HS-PS3-1

NGSS.HS-PS3-4

A pot of 2400g of water at a temperature of 25˚C is heated on a stove until the water boils (100˚C).  The specific heat of water is 4.18 J/(g˚C).
Determine the heat energy needed to heat the water in the pot to boiling.

• 133.76J
• 43,062.2J
• 752,400J
• 1,003,200J

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

Calculate the energy transferred when raising the temperature of 16kg of water by 3˚C (c=4,186 J/(kg K))

• 785 J
• 1.26*10^5 J
• 2.2 kJ
• 2.0*10^5 J

Tags

NGSS.HS-PS3-1

What does Q represent in:

Q=m*c*ΔT

• Energy Flow

• Mass

• Specific Heat Capacity

• Change in temperature

50 g of a metal absorbs 900 J when it is heated from 25 °C to 85 °C. What is the specific heat of the metal?

• 0.7 J/g°C

• 0.3 J/g°C

• 1.2 J/g°C

• 2.0 J/°C

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4