Question

A 1000 g chunk of copper is measured to have an initial temperature of 23°C. If the copper absorbs 23,100J of energy, what was the final temperature of the copper? The specific heat of copper is 0.385 J/g°C. (Note: Make sure you use the lowest significant figures in your answer.

A) 43°C

B) 48°C

C) 53°C

D) 58°C

Answer 1

The final temperature of the copper is 83°C. Since none of the provided answer choices match 83°C, none of the options A, B, C, or D are correct.

Step-by-step explanation:

In order to find the final temperature of the copper, we can use the equation: q = mcΔT

where:

- q is the amount of energy absorbed by the copper (23,100 J)

- m is the mass of the copper (1000 g)

- c is the specific heat of copper (0.385 J/g°C)

- ΔT is the change in temperature

First, we can rearrange the equation to solve for ΔT: ΔT = q / (mc)

Now, substitute the given values into the equation:

ΔT = 23,100 J / (1000 g * 0.385 J/g°C)

Simplifying this expression: ΔT = 23,100 J / 385 J/°C

ΔT = 60°C

Therefore, the final temperature of the copper is 23°C + 60°C = 83°C.

As none of the provided answer choices match 83°C, none of the options A, B, C, or D are correct.