1. The problem statement, all variables and given/known data A piece of iron weighed at 120 grams at 95.0 degrees Celcius is added to 750ml water of 25.0 degrees Celcius. What is the final temperature of the water when it is equilibrated? Assume the dentisy of water is 1 g/ml. (Specific heat of water is 4.184 and specific heat of iron is .449). 2. Relevant equations q=mc(delta t). In this case the q of iron is equal to the q of water. 3. The attempt at a solution Here is my setup: 120*.449(x-95)=750*4.184(x-25) Solving: 53.88x-5118.6=3138x-78450 53.88x=3138x-73331.4 -3084.12x=-73331.4 x=23.85 I know this is wrong, but I'm not sure if it's because I set this up wrong or did my calculations incorrectly.
I don't understand what you mean. I know that 23.85 implies that the temperature decreased for both the iron and water, and that is wrong.
I think I forgot the qin=-qout concept. Let me try again. 120*.449(x-95)=-750*4.184(x-25) 53.88x-5118.6=-3138x+78450 3191.88x=83568.6 x=26.18 degrees Celcius Is this what you were referring to?
Almost, if one thing is cooling from 95deg to x then the change in T is (95-x) then if the other is heating form 25 to X the change must be (x-25) which gives the different signs. Putting a minus on one side is the same thing (or at least has the same effect)
I thought that in order to do the equation correctly, one must always subtract the initial temperature from the final temperature.