A 6.75-g sample of gold (specific heat capacity = 0.130 J/g °C) is heated using 55.8 J of energy. If the original temperature of the gold is 25.0°C, what is its final temperature?
A) 88.6 °C
B) 38.6 °C
C) 76.9 °C
D) 73.6 °C
E) 63.6 °C

Question

Quizplus · Accepted Answer

Explanation:The change in temperature (ΔT) of the gold can be calculated using the equation:ΔT = Q / (m * c)where Q is the energy added, m is the mass of the gold, and c is the specific heat capacity of the gold.Plugging in the given values, we get:ΔT = 55.8 J / (6.75 g * 0.130 J/g °C) = 63.6 °CTherefore, the final temperature of the gold is 25.0 °C + 63.6 °C = 88.6 °C.

A 675-G Sample of Gold (Specific Heat Capacity = 0