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I don't understand....?
A 4.50-g nugget of pure gold absorbed 276j of heat. What is the final temperature of the gold if the initial temperature was 2.50 degrees Celsius? The specific heat of gold is 0.129j/(g* degrees Celsius)
My teacher taught me only how to solve how much heat is absorbed/released and how to find specific heat capacity. But initial temperature and final temperature? What is that? It seems all too complicated. I don't understand the question at all and can't solve it... Please help!
1 Answer
- kentuckyLv 610 years agoFavorite Answer
The energy equation Q = mCΔT says the amount of heat is equal to the product of the mass, the specific heat capacity and the change in temperature (ΔT is one variable). Now given any three of these variables, you can solve for the fourth. So, given 4.50 g and 0.129 J/g*deg C and 276 J, you can rearrange to ΔT = Q/mC to get the change in temperature. Now since you know that heat is absorbed, you should know that the temperature will go up. Add the ΔT to 2.50 deg C to get the final temp.
