Question

A 6.50-g sample of copper metal at 25.0°C is heated by the addition of 84.0 J of energy. The final temperature of the copper is ________°C. The specific heat capacity of liquid water is 0.38 J/g-K.

Answer 1

Answer:

Final temperature of the copper is 59 degrees Celsius

Explanation:

It is given that,

Mass of the sample of copper metal, m = 6.5 g

Initial temperature of the metal, $T_i=25^{\circ}\ C=298\ K$

Heat generated, Q = 84 J

The specific heat capacity of liquid water is 0.38 J/g-K

Let $T_f$ is the final temperature of the copper. It can be calculated using the definition of specific heat of any substance. It is given by :

$Q=mc\Delta T$

$Q=mc(T_f-T_i)$

$T_f=\dfrac{Q}{mc}+T_i$

$T_f=\dfrac{84}{6.5\times 0.38}+298$

$T_f=332\ K$

or

$T_f=59^{\circ}C$

So, the final temperature of the copper is 59 degrees Celsius. Hence, this is the required solution.

Answer 2

The final temperature of a 6.50g sample of copper metal at 25.0°C heated by the addition of 84.0 J of energy is 59.01°C.

How to calculate final temperature?

The final temperature of a substance can be calculated using the following formula:

Q = m × c × ∆T

Where;

• Q = quantity of heat absorbed or released
• m = mass of the substance
• c = specific heat capacity
• ∆T = change in temperature

84 = 6.5 × 0.38 × (T - 25)

84 = 2.47T - 61.75

84 + 61.75 = 2.47T

T = 145.75 ÷ 2.47

T = 59.01°C

Therefore, the final temperature of a 6.50g sample of copper metal at 25.0°C heated by the addition of 84.0 J of energy is 59.01°C.

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