Question

Question #0ee35

Answer 1

The specific heat of your metal is `0.73"J"/("g"^@"C")`.

Explanation:

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

`q = m * c * DeltaT`, where

`q` - the heat supplied to the metal;
`m` - the mass of the metal;
`c` - the specific heat of the metal;
`DeltaT` - the change in temperature, defined as the final temperature minus the initial temperature.

In your case, you know that the temperature of a 17.5-g sample of an unknown metal increased by `3.0^@"C"` upon absorption of 38.5 J of heat.

Since the temperature increased by `3.0^@"C"`, you know that

`T_"final" - T_"initial" = 3.0^@"C" = DeltaT`

This means that the specific heat of the metal is

`c = q/(m * DeltaT)`

`c = (38.5"J")/("17.5 g" * 3.0^@"C") = 0.7333"J"/("g" ^@"C")`

Rounded to two sig figs, the number of sig figs you gave for the change in temperature, the naswer will be

`c = color(green)(0.73"J"/("g"^@"C")`