Question

Type the correct answer in each box. Express your answer to four significant figures. The temperature of 15.71 grams of gold rises from 32°C to 1,064°C, and then the gold melts completely. If gold’s specific heat is 0.1291 joules/gram degree Celsius and its heat of fusion is 63.5 joules/gram, how much energy is gained by the gold? The gold gained a total of _____ joules of energy.

Answer 1

The gold gained a total of 30398.39 J of energy through a temperature change and phase change.

Step-by-step explanation:

In this problem, we can calculate the energy gained by the gold by using the formula Q = mcΔT, where Q is the energy gained, m is the mass of the gold, c is the specific heat of gold, and ΔT is the change in temperature. We can first calculate the energy gained through the temperature change and then add the energy gained through the phase change.

Using the formula, Q = mcΔT, for the temperature change: Q = (15.71 g)(0.1291 J/g°C)(1064°C - 32°C) = 20411.54 J.

Using the formula, Q = mΔHf, for the phase change: Q = (15.71 g)(63.5 J/g) = 9986.85 J.

Adding both values together, the gold gained a total of 20411.54 J + 9986.85 J = 30398.39 J of energy.