$\mathbf{q}\mathbf{=}\mathbf{mc}\mathbf{\u2206}\mathbf{T}$

- (+) → gains heat
- (-) → loses heat

**-q _{coffee }= +q_{ice}**

When ice melts at 0°C:

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{n}}{\mathbf{\times}}{{\mathbf{\Delta H}}}_{{\mathbf{fusion}}}}\phantom{\rule{0ex}{0ex}}$

${\mathbf{q}}_{\mathbf{ice}}\mathbf{=}\mathbf{mc}\mathbf{\u2206}\mathbf{T}\mathbf{+}\mathbf{n}\mathbf{\u2206}{\mathbf{H}}_{\mathbf{fusion}}$

An ice cube of mass 9.0 g at temperature 0^{o}C is added to a cup of coffee, whose temperature is 95 ^{o}C and which contains 130 g of liquid. Assume the specific heat capacity of the coffee is the same as that of water. The heat of fusion of ice (the heat associated with ice melting) is 6.0 kJ/mol.

Find the temperature of the coffee after the ice melts. Express your answer using two significant figures.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Heating and Cooling Curves concept. You can view video lessons to learn Heating and Cooling Curves. Or if you need more Heating and Cooling Curves practice, you can also practice Heating and Cooling Curves practice problems.

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