Question

Question #39f99

Answer 1

Here's what I got.

Explanation:

A substance's specific heat tells you how much heata is needed to increase the temperature of `"1 g"` of that substance by `1^@"C"`.

The equation that establishes a relationship between heat absorbed and increase in temperature looks like this

`color(blue)(q = m * c * DeltaT)" "`, where

`q` - the heat absorbed by the sample
`m` - the mass of the sample
`c` - the specific heat of the substance
`DeltaT` - the change in temperature, defined as the final temperature minus the initial temperature

In your case, you know that

• your metal sample has a mass of `"15.0 g"`
• the temperature of the sample increases from `25.00^@"C"` to `32.00^@"C"` after adding `"178.1 J"` worth of heat to it

So, plug in your values and solve for `c`, the specific heat of the metal

`c = q/(m * DeltaT)`

`c = "178.1 J"/("15.0 g" * (32.00 - 25.00)^@"C") = color(green)(1.70"J"/("g" ""^@"C"))`

SIDE NOTE This is a very high value to get for the specific heat of a metal, so make sure that you double-check the values you were given for heat absorbed, mass, and temperature change.

The way I see it, either the mass of the sample or the temperature change are too small, or the amount of heat absorbed is too high.