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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: OrganicH2O on May 20, 2019, 06:32:22 PM

Title: Calorimetry question
Post by: OrganicH2O on May 20, 2019, 06:32:22 PM

I am trying to solve the following problem. I already have the answer, it is 0.38 J/(g x k)

"When 1.0 × 10^2 g of an unknown metal
at 80.0°C is placed in a calorimeter containing 1.0 × 10^2 g of water, the temperature of the water rises from 20.0°C to 25.0°C. Given that the specific heat of water is 4.184 J/g•K, what is the specific heat of the metal?" 

I am trying to solve it by using the idea: qH₂O = -qMetal , and therefore msΔT = -(msΔT), where one side is for water and the other side is for the metal.

The problem is that it seems like I am missing two variables, when I essentially only have one equation. I do not know the specific heat of the metal, and I also do not know the change in temperature of the metal. Doesn't the change in temperature of the metal depend on the specific heat of the metal?

This question is from an MTEL practice exam (high school teacher's license) that I am helping somebody with. Is there a typo or something missing? Is there a second equation I should be using to account for the two variables I do not know? Or am I missing something else?

Title: Re: Calorimetry question
Post by: Borek on May 21, 2019, 03:05:24 AM

Can the final temperature of the metal be different from the temperature of water?