A piece of iron (400. g) is heated in a flame and then plunged into a beaker containing 1.00 kg of water. The original temp of the water was 20.0 degrees Celcius, but it is 32.8 degrees after the iron bar is put in and thermal equilibrium is reached. What was the original temp of the hot iron bar?
equation: mass * enthalpy * change in temp
water: 4.184 J/(g*C)
iron: 0.451 J/(g*C)
I can calculate the heat of the water, but when I try to set up the equation for the iron, I get two variables:
q(Fe) = 400. g * .451 J/(g*C) * (32.8 C - initial temp)
did i do something wrong? or how can i solve this?
2006-10-26
17:09:44
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1 answers
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asked by
Anonymous
in
Chemistry