# How many calories are absorbed when 500 grams of water (1 cal/g c) is heated from 50 to 100 degrees Celsius?

##### 1 Answer

#### Answer:

#### Explanation:

You know that the **specific heat** of a substance tells you the amount of heat needed to increase the temperature of

In your case, water is said to have a specific heat equal to

#c_"water" = "1 cal g"^(-1)""^@"C"^(-1)#

This means that in order to increase the temperature of

So, how much heat would be needed to increase the temperature of

#500 color(red)(cancel(color(black)("g"))) * overbrace("1 cal"/(1color(red)(cancel(color(black)("g")))))^(color(blue)("for 1"^@"C")) = "500 cal"#

This means that in order to increase the temperature of

#100^@"C" - 50^@"C" = 50^@"C"#

you need to provide it with

#50 color(red)(cancel(color(black)(""^@"C"))) * overbrace("500 cal"/(1color(red)(cancel(color(black)(""^@"C")))))^(color(blue)("for 500 g")) = "25,000 cal" = color(darkgreen)(ul(color(black)("30,000 cal")))#

The answer **must** be rounded to one **significant figure**, the number of sig figs you have for your values.

Keep in mind that this much heat is needed in order to get *liquid* at *liquid* at