Question

Brass is an alloy made from copper and zinc. A 590 g brass candlestick has an initial temperature of 98.0°C. If 21,100 J of

energy is removed from the candlestick to lower its temperature to 6.8°C, what is the specific heat of brass?
4.012 J/gºC
0.526 J/gºC
0.392 J/gºC
52.59 J/gºC

Answer 1

To determine the specific heat of brass, we can use the formula:

q = m * c * ΔT

where:
q = energy transferred (in joules)
m = mass of the brass (in grams)
c = specific heat of brass (in J/gºC)
ΔT = change in temperature (final temperature - initial temperature) in ºC

In this case, we know the following values:
q = -21,100 J (energy removed from the candlestick)
m = 590 g (mass of the brass)
ΔT = (6.8°C - 98.0°C) = -91.2°C (change in temperature)

Plugging in these values, we can solve for c:

-21,100 J = 590 g * c * (-91.2°C)

Dividing both sides of the equation by (590 g * -91.2°C):

c = -21,100 J / (590 g * -91.2°C)

Calculating the result gives us:

c ≈ 0.392 J/gºC

Therefore, the specific heat of brass is approximately 0.392 J/gºC. The correct option from the given choices is 0.392 J/gºC.