A 20g piece of lead absorbs 566 joules of heat and its temperature changes from 35 oC to 195 oC. Calculate the specific heat.

40g of water is heat at 40 oC and the temperature rise to 75 oC. What is the amount of heat needed for the temperature to rise? (specific heat of water is 4.184 J/g oC)

Graphite has a mass of 50g and a specific heat of 0.420 J/g oC. If graphite is cooled from 50 oC to 35 oC, how much energy was lost?

Iron has a specific heat of 0.712 J/g oC. A piece of iron absorbs 3000J of energy and undergoes a temperature change totaling 50 oC, What is the mass of iron?

If 400g of an unknown solution at 70 oC loses 7500 J of heat, what is the final temperature of the unknown solution. The unknown solution has a specific heat of 4.184 J/g oC.

How many grams of water would require 9500J of heat to raise the temperature from 50 oC to 100 oC

Question 1: 0.2J / (gºC) Question 2: 6,000J Question 3: 300J Question 4: 80g Question 5: 74ºC Question 6: 50g

Explanation:

Question 1. A 20g piece of lead absorbs 566 joules of heat and its temperature changes from 35º oC to 195º C. Calculate the specific heat.

The thermal energy equation is:

Q = m * C * ΔT

Substitute and solve for C:

566J = 20g * C * (195ºC - 35ºC) C = 566J / (20g * 160ºC) C = 0.177 J / (gºC) ≈ 0.2J / (gºC)

You must round to one significant figure because one factor has one significant figure).

Qustion 2. 40g of water is heat at 40ºC and the temperature rise to 75ºC. What is the amount of heat needed for the temperature to rise? (specific heat of water is 4.184 J/gºC)

Use the thermal energy equation again:

Q = m * C * ΔT

Substitute and compute:

Q = 40g * 4.184 J/gºC * (75ºC - 40ºC) Q = 5,857.6J

Round to one significant figure: 6,000J

Question 3. Graphite has a mass of 50g and a specific heat of 0.420 J/gºC. If graphite is cooled from 50ºC to 35ºC, how much energy was lost?

Q = m * C * ΔT Q = 50g * 0.420J/gºC * (35ºC - 50ºC) Q = 315J

Round to one significant figure (because 50g has one significant figure)

Q = 300J

Question 4. Iron has a specific heat of 0.712 J/gºC. A piece of iron absorbs 3000J of energy and undergoes a temperature change totaling 50ºC, What is the mass of iron?

Q = m * C * ΔT

Solve for m:

m = Q / (C * ΔT)

Substitute and compute:

m = 3,000J / (0.712J/gºC * 50ºC) m = 84.26 g ≈ 80 g (rounded to one significant figure, because the factor 3,000J has one significant figure).

Question 5. If 400g of an unknown solution at 70ºC loses 7500 J of heat, what is the final temperature of the unknown solution. The unknown solution has a specific heat of 4.184 J/gºC.

Q = m * C * ΔT

Q is negative, since it is released.

Substitute and solve for T:

- 7,500J = 400g * 4.184J/gºC * (T - 70ºC)

T = - 7500J / 400g * 4.184J/gºC) + 70ºC

T = 74ºC

If you round to one significant figure you cannot tell the temperature difference, thus leave two significant figures.

Question 6. How many grams of water would require 9500J of heat to raise the temperature from 50ºC to 100ºC

Q = m * C * ΔT

Subsitute:

9,500J = m * 4.184J/gºC * (100ºC - 50ºC)

Solve for m and compute:

m = 9,500J / (4.184J/gºC * 50ºC)

m = 45g

Since the temperatures indicate one singificant figure, the mass should be rounded to one significant figure:

m = 50g.