# Question #3269e

##### 1 Answer

Here's what I got.

#### Explanation:

I'm going to assume that you're interested in determining the amount of heat needed to convert **liquid water** at its normal melting point of **liquid water** at its normal boiling point of

In other words, I will assume that you don't have to go from **solid water** at **water vapor** at *phase change* is involved here.

Now, the **specific heat** of water, which tells you the amount of heat needed to increase the temperature of

In your case, you would need

#89.5 color(red)(cancel(color(black)("g"))) * "4.18 J"/(1color(red)(cancel(color(black)("g"))) * 1^@"C") = "374.11 J"""^@"C"^(-1)#

in order to increase the temperature of your sample of water. This value tells you that every *your sample* requires

You can thus say that a change in temperature of

#100^@"C" - 0^@"C" = 100^@"C"#

will require

#100 color(red)(cancel(color(black)(""^@"C"))) * overbrace("374.11 J"/(1color(red)(cancel(color(black)(""^@"C")))))^(color(blue)("for 89.5 g of water")) = "37,411 J"#

of heat. Rounded to three **sig figs**, the number of significant figures you have for the mass of water, and expressed in *kilojoules*, the answer will be

#color(darkgreen)(ul(color(black)("heat needed = 37.4 kJ")))#