# Question #44228

##### 1 Answer

#### Explanation:

All you have to do here is use the equation the establishes a relationship, in your case, between heat gained and increase in temperature

#color(blue)(q = m * c * DeltaT)" "# , where

*final temperature* minus *initial temperature*

So, you know that copper has a specific heat of

#c_"copper" = 0.385"J"/("g" ""^@"C")#

So, what does a substance's specific heat tell you?

Well, it tells you how much heat is needed to increase the mass of a

Now, if you have a **bigger mass**, you'd need more heat to increase its temperature by

If you also want to increase its temperature by **more than**

In your case, the change in temperature will be

#DeltaT = 324.3^@"C" - 20.5^@"C" = 303.8^@"C"#

This means that the amount of heat you'd need will be equal to

#q = 6.22 color(red)(cancel(color(black)("g"))) * 0.385"J"/(color(red)(cancel(color(black)("g"))) color(red)(cancel(color(black)(""^@"C")))) * 303.8color(red)(cancel(color(black)(""^@"C"))) = "727.51 J"#

Rounded to three sig figs, the answer will be

#q = color(green)("728 J")#