A 2.74g sample of a substance assumed to be pure gold is warmed to 80.0C and submerged in to 15.2 g of water, initially at 24.7 C. The final temperature of the mixture is 25.30C. What is the heat capacity of the substance? could this substance be pure gold?
m(water) = 15.2 g
T(water) = 24.7 oC
C(water) = 4.184 J/goC
m(gold) = 2.74 g
T(gold) = 80.0 oC
C(gold) = to be calculated
We will be using heat conservation equation
use:
heat lost by gold = heat gained by water
m(gold)*C(gold)*(T(gold)-T) = m(water)*C(water)*(T-T(water))
2.74*C(gold)*(80.0-25.3) = 15.2*4.184*(25.3-24.7)
149.878*C(gold) = 38.1581
C(gold)= 0.255 J/goC
Answer: 0.255 J/goC
Actual specific heat capacity of gold is 0.129 J/goC
So, this can’t be pure gold
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