A piece of iron (C = 0.449 J/g°C)and a piece of gold (C = 0.128 J/g°C)have identical masses.If the iron has an initial temperature of 498 K and the gold has an initial temperature of 298 K,which of the following statements is TRUE of the outcome when the two metals are placed in contact with one another? Assume no heat is lost to the surroundings.

Question

Quizplus · Accepted Answer

The final temperature of the two metals will lie somewhere in between 498 K and 298 K because there will be thermal energy exchange between the two metals. However, since iron has a much greater specific heat capacity than gold, it will take longer for iron to exchange its thermal energy with gold than vice versa. This means that at thermal equilibrium, the iron will lose heat and the gold will gain heat, resulting in a final temperature closer to 498 K than to 298 K. Therefore, choice D is the correct statement. Choice A is not true because the final temperature will not necessarily be exactly halfway between the two initial temperatures. Choice B is not true because it is based on the erroneous assumption that having a smaller specific heat capacity means a metal will have a lower final temperature. Choice C is not true because while the thermal energy transferred will be equal, the final temperature of the two metals will not be the same.

A Piece of Iron (C = 0