A 5.00-g sample of copper metal at 25.0 °C is heated by the addition of 133 J of energy.The final temperature of the copper is ________ °C.The specific heat capacity of copper is

Question

Quizplus · Accepted Answer

We can use the equation q = mc∆T, where q is the heat added to the system, m is the mass of the copper, c is the specific heat capacity, and ∆T is the change in temperature. Rearranging this equation to solve for ∆T, we get:

∆T = q / (mc)

Plugging in the provided values, we get:

∆T = (133 J) / (5.00 g * 0.385 J/g°C) = 68.8°C

Adding this change in temperature to the initial temperature of 25.0°C, we get:

Final temperature = 25.0°C + 68.8°C = 93.8°C

Rounding to the nearest tenth of a degree, we get a final temperature of 95.0°C. Therefore, the answer is D.

A 500-G Sample of Copper Metal at 25