Question

Question #95ca2

Answer 1

`"9,900 J"`

Explanation:

Your goal here is to figure out how much heat is needed to increase the temperature of `"55 g"` of water by

`87^@"C" - 44^@"C" = 43^@"C"`

The key here is the specific heat of water, which tells you the amount of heat needed to increase the temperature of `"1 g"` of water by `1^@"C"`.

Use the specific heat of water to determine the energy needed to increase the temperature of `"55 g"` of water

`55 color(red)(cancel(color(black)("g"))) * overbrace("4.184 J"/(1color(red)(cancel(color(black)("g"))) * 1^@"C"))^(color(blue)("the specific heat of water")) = "230.12 J"""^@"C"^(-1)`

This tells you that in order to increase the temperature of `"55 g"` of water by `1^@"C"`, you need to provide `"230.12 J"`.

Consequently, you can say that in order to increase the temperature of the sample by `43^@"C"`, you need

`43 color(red)(cancel(color(black)(""^@"C"))) * overbrace("230.12 J"/(1color(red)(cancel(color(black)(""^@"C")))))^(color(blue)("for 55 g of water")) = color(darkgreen)(ul(color(black)("9,900 J")))`

of heat. The answer is rounded to two sig figs.