# Question #f51b9

##### 1 Answer

#### Explanation:

In order to be able to answer this question, you need to know the **specific heat** of silver.

#c_"Ag" = "0.240 J g"^(-1)""^@"C"^(-1)#

http://www2.ucdsb.on.ca/tiss/stretton/database/specific_heat_capacity_table.html

Now, the specific heat of silver tells you the amount of energy needed to increase the temperature of

You can thus say that if you add

In your case, the temperature of the sample must increase by

#78^@"C" - 15^@"C" = 63^@"C"#

so use the specific heat to calculate the amount of heat needed to increase the temperature of a sample of silver by

#63 color(red)(cancel(color(black)(""^@"C"))) * "0.240 J"/("1 g" * 1 color(red)(cancel(color(black)(""^@"C")))) = "15.12 J g"^(-1)#

This tells you that in order to increase the temperature of silver by **for every**

You can thus say that your sample will require

#35 color(red)(cancel(color(black)("g"))) * overbrace("15.12 J"/(1color(red)(cancel(color(black)("g")))))^(color(blue)("for a 63"""^@"C increase in temperature")) = color(darkgreen)(ul(color(black)("530 J")))#

The answer is rounded to two **sig figs**, the number of sig figs you have for your values.