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

- (+) → 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.

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