Question

A 6.22-kg piece of copper metal is heated from 20.5 °C to 324.3 °C. The specific heat of Cu is 0.385 Jg-1°C-1.a.Calculate the heat absorbed (in kJ) by the metal.b.How close is this heat capacity to the expected heat capacity at the classical limit?

Answer 1

Answer:

a) 727.5 kJ

Explanation:

Step 1: Data given

Mass of the piece of copper = 6.22 kg

Initial temperature of the copper = 20.5 °C

Final temperature of the copper = 324.3 °C

Specific heat of copper = 0.385 J/g°C

Step 2:

Q = m*c*ΔT

⇒ with Q = heat transfer (in J)

⇒ with m = the mass of the object (in grams) = 6220 grams

⇒ with c = the specific heat capacity = 0.385 J/g°C

⇒ with ΔT = T2 -T1 = 324.3 -  20.5 = 303.8

Q = 6220 grams * 0.385 J/g°C * 303.8 °C

Q = 727509.9 J = 727.5 kJ

b) This heat capacity is the heat capacity given for a copper at a temperature of 25°C

Answer 2

The heat absorbed  by the metal and the heat capacity is mathematically given as

Q= 727.5 kJ

The Heat capacity is  25°C

What is the heat absorbed (in kJ) by the metal and the heat capacity?

Question Parameter(s):

A 6.22-kg piece of copper metal is heated from 20.5 °C to 324.3 °C. The specific heat of Cu is 0.385 Jg-1°C-1.a.

Generally, the equation for the Heat is mathematically given as

Q = m*c*dT

Therefore

dT = T2 -T1

dT= 324.3 -  20.5

dT= 303.8

Hence

Q = 6220 * 0.385  * 303.8

Q= 727509.9 J

Q= 727.5 kJ

In conclusion, heat capacity is, copper at a temperature of 25°C

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