Question

If 45.0 mL of ethanol (density=0.789 g/mL) initially at 9.0 C is mixed with 45.0 mL of water (density=1.0 g/mL) initially at 28.6 C in an insulated beaker, and assuming that no heat is lost, what is the final temperature of the mixture?

 

I tried many times in trying to get the answer, but I keep getting it wrong. I appreciate who answers this writes it step by step. Thank you.

Answer 1

Given data Volume of ethanol, 45 mL Density of ethanol, P 0.789 g/mL Volume of water. ,245 mL Density of water, Py 1g/mL Initial temperature of ethanol, T9 C Initial temperature of water, T 28.6 C Heat capacity of water, cw-418 J/g-K Heat capacity of ethanol, ct 2.3 J/g-K There is no loss of heat to surrounding Hence, the heat lost by water is equal to the heat gained by ethanol. ost gained Substitute the values 1x 45×4.18(28.6-T)-(0.789% 45) x2.3(-9) 4.18(286-5)=1.8147(7-9) T, 22.67°c Hence, the final temperature of mixture is 22.67°C