16 Heat

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?  (show your work)

• 25g
• 30g
• 20g
• 50g

For the formula:
 Q= m c ∆T
The  units for specific heat are:

• g /J C
• °C/g J
• kJ/g
• J/g°C

Tags

NGSS.HS-PS3-1

What is energy?

•  the ability to do work
• how much power a system has.
•  the flow of heat
• how awake a person feels

If I have 2 blocks of Aluminium (one of 1kg and one of 10 kg) and heat them up.
Which one heats up the fastest.

• 1 kg
• 10 kg
• They both heat up at the same speed
• They don't heat up.

Tags

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

Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same thermal energy.  What material would be the coolest after being heated?

• Copper
• Carbon Steel
• Zinc
• Stainless Steel

Tags

NGSS.HS-PS3-4

How many Joules of energy are required to change 10 gram of water from 20 C to 90 C?

• 1400 J
• 2800 J
• 210,000 J
• 1,400,000 J

Tags

NGSS.HS-PS3-1

NGSS.HS-PS3-4

A 9.5 kg outdoor copper structure heats up during the day from 24 degrees C to 78 degrees C. How much energy was absorbed? Note: copper has a specific heat of 390 J/kg C

• 100,000 J
• 247,000 J
• 200,070 J
• 235,000 J

How much heat is required to completely change 5.3 g of water from solid to liquid?

• 334 J/g
• 1770 J
• 63 J
• 1800 J

How much heat is required to change 10.2 g of water from -11.2^OC to 53.4^OC?

• 27.5 kJ
• 59,178 J
• 5,920 J
• 2,750 J