Question

If I added 10 kJ of heat to a 100 g cube of copper and 10 kJ of heat to a 100 g cube of aluminum, which cube would experience a greater change in temperature. Explain your answer in terms of specific heat.

Answer 1

Answer:

The cube of copper

Explanation:

Cube of copper has a lower specific heat than the cube of aluminum. This pretty much shows that the lower specific heat, the higher change in temp.

(yeah i just found out how to do it like a minute ago cos its on my hw)

Answer 2

A cube of copper would experience a greater change in temperature in comparison with a cube of aluminum.

Given the following data:

• Quantity of heat = 10 kJ = 10,000 Joules

• Mass of copper cube = 100 g

• Mass of aluminum cube = 100 g

• Specific heat capacity of aluminum = 0.89 J/g°C

• Specific heat capacity of copper = 0.39 J/g°C.

To determine which cube would experience a greater change in temperature:

Mathematically, quantity of heat is given by the formula;

$Q = mc\theta$

Where:

• Q represents the quantity of heat.

• m represents the mass of an object.

• c represents the specific heat capacity.

• ∅ represents the change in temperature.

Making change in temperature (∅) the subject of formula, we have:

$\Theta = \frac{Q}{mc}$

For copper cube:

$\theta = \frac{10000}{100(0.39)}\\\\\theta = \frac{10000}{39}$

Change in temperature ($\theta$) = 256.41°C

For aluminum cube:

$\theta = \frac{10000}{100(0.89)}\\\\\theta = \frac{10000}{89}$

Change in temperature ($\theta$) = 112.36°C

Based on the above calculations, we can deduce and conclude that a cube of copper would experience a greater change in temperature in comparison with a cube of aluminum.

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