# Question 95ca2

Sep 24, 2017

#### Answer:

$\text{9,900 J}$

#### Explanation:

Your goal here is to figure out how much heat is needed to increase the temperature of $\text{55 g}$ of water by

${87}^{\circ} \text{C" - 44^@"C" = 43^@"C}$

The key here is the specific heat of water, which tells you the amount of heat needed to increase the temperature of $\text{1 g}$ of water by ${1}^{\circ} \text{C}$.

Use the specific heat of water to determine the energy needed to increase the temperature of $\text{55 g}$ 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 $\text{55 g}$ of water by ${1}^{\circ} \text{C}$, you need to provide $\text{230.12 J}$.

Consequently, you can say that in order to increase the temperature of the sample by ${43}^{\circ} \text{C}$, you need

$43 \textcolor{red}{\cancel{\textcolor{b l a c k}{\text{^@"C"))) * overbrace("230.12 J"/(1color(red)(cancel(color(black)(""^@"C")))))^(color(blue)("for 55 g of water")) = color(darkgreen)(ul(color(black)("9,900 J}}}}$

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