1. The problem statement, all variables and given/known data Your 200-g cup of tea is boiling-hot. About how much ice should your add to bring it down to a comfortable sipping temperature of65°C . Assume that the ice is initially at−15°C . The specific heat capacity of ice is 0.5cal g⋅°C , for water is 1 cal g⋅°C. The latent heat for melting ice is 80cal g. 2. Relevant equations Equation for latent heat: L=Q/m 3. The attempt at a solution First I need to find the heat lost by the water. This is done using: Q=cwmwΔT → (1 cal g⋅°C)(200 g)(65 C - 100 C) Q=-7000 calories Assuming no heat is lost to anything else during the process, Qlost = Qgained So the ice cube gains the heat lost by the water, or 7000 calories. Here is where I am stuck. I tried using the latent heat equation directly (L=Q/m → m=Q/L) using the latent heat of melting ice a 80 cal/g, but this gave me the incorrect answer. How does one figure out the mass? I tried subbing in the specific heat capacity for Q in the latent heat eqn, but then my masses cancelled. So that didn't work.