rare coin dealers
Chem Question……confused….?
A coin dealer, offered a rare silver coin, suspected that it might be a counterfeit nickel copy. The dealer heated the coin, which weighed 14.0 g to 100°C in boiling water and then dropped the hot coin into 28.5 g of water at T = 17.0°C in an insulated coffee-cup, and measured the rise in temperature. If the coin was really made of silver, what would the final temperature of the water be (in °C)? (for nickel, s = 0.445 J/g-degC; for silver, s = 0.233 J/g-degC )
I understand that they are heating the coin to 100 celcius and puttin it in water and based on its specific heat, it would lose a certain amount of heat, but how do u do this problem. I don’t know the q of reaction.
you have two proposed qs – one for silver and one for nickel
start with the relevant facts:
its 4.184 calories /joule
1 calorie can heat 1 g of water 1 deg C
every degree change in the water is 28.5 calories (for 28.5 g of water)
or 6.811 J/degC
for the coin the energy released is = (100 – Tf) * q * 14.0 g
for the water the energy is = (Tf – 17.0) * 28.5 /4.185
since these two energies are equal:
(Tf – 17.0) * 6.811(J/degC) = (100.0 – Tf) * q * 14.0g
plug both qs into the equation to get the two final temperatures
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