24.7 of ethanol (density =0.789 ) initially at 5.0 is mixed with 30.6 of water (density = 1.0 ) initially at 24.6 in an insulated beaker.

Question

24.7  of ethanol (density =0.789 ) initially at 5.0 is mixed with 30.6  of water (density = 1.0 ) initially at 24.6 in an insulated beaker.

anonymous · Answer

This is what I have so far: 24.7mL*(0.789g/mL)*[2.42J/(g*Celsius)]*[Tf-5.0Celsius]+30.6mL*(1.0g/mL)*[4.184J/(g*Celsius)]*[Tf-24.6Celsius]

anonymous · Answer

Assuming that no heat is lost, what is the final temperature of the mixture?

jfraser · Answer

replace the "+" with a "=", and you're all set. Solve for Tf.

It's all based on the conservation of energy. Whatever energy the water loses must be gained by the ethanol, producing different temperature changes, but the same final temperature.