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An insulated Thermos contains 144 cm3 of hot coffee at 89 °C. You put a 12.0 g ice cube at its melting point t?

An insulated Thermos contains 144 cm3 of hot coffee at 89 °C. You put a 12.0 g ice cube at its melting point to cool the coffee. By how many degrees has your coffee cooled once the ice has melted and equilibrium is reached? Treat the coffee as though it were pure water and neglect energy exchanges with the environment.

I don’t have all the values to look up, so I’ll just leave my answer in variable form.

Let T = final temperature of the mixture (C)

Energy gained by ice = m_ice * (h_sf + cpw*T)
Energy lost by coffee = ρ_w*V_coffee*cpw*(89 – T)

set them equal and solve for T.

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