Cumalative Thermochemistry Problem Help

I have an idea of how to begin this one, but become lost quite soon into the problem.
Question: If 45.0 mL of ethanol (density= 0.789g/mL) initially at 6.0C is mixed with 45.0 mL of water (density = 1.0g/mL) initially at 28.1C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?
What I Believe So Far: I believe I would first need to obtain the amounts of ethanol and water in grams. So, assuming this is correct, I just convert using the densities. I obtain 35.51g of Ethanol and 45g of Water. Secondly, would I not need to get the Heat Capacities of both Ethanol and Water? I’m not sure, but I would think I need to, but if not, then this is where I become lost, but if so, Ethanol’s is 2.438J/gC and Water’s is 4.180J/gC. Then I would assume I need to find out how much energy each substance requires, which is 5.12 x 10^3 for Water, and 5.19 x 10^2 for Ethanol. Then I’m lost, assuming this is even correct so far.
Can anyone help lead me in the direction to solving this problem?
Thank you.
Answer #1
anyone?