If you have 50.0 g samples of each of the 5 metals and water, and you add 400 cal of energy to each, which substance will have the largest resulting temperature change? (Use the metals listed in problem 2 to answer this problem.)

Question

Casey

Chemistry

3 August, 16:07

If you have 50.0 g samples of each of the 5 metals and water, and you add 400 cal of energy to each, which substance will have the largest resulting temperature change? (Use the metals listed in problem 2 to answer this problem.)

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Answers (1)

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Ronnie Blevins · Answer 1

The largest temperature change corresponds to the metal with the lowest specific heat

Explanation:

The metals listed in problem 2 are missing, so I will answer this question in general terms.

The formula that relate the heat absorbed or rejected from a body (q), the mass of the body (m), its specific heat (cp), and the temperature change (ΔT) is:

q = m*cp*ΔT

Given that all materials receive the same amount of heat and have the same mass then we can rewrite the formula as follows:

q/m = cp*ΔT = k

where k is some constant (the same for the 5 cases). Therefore, the greater the cp, the lower the ΔT, and viceversa.