Question

1.0 gram of copper and 1.0 gram of silver were both heated to 100 °C and then dropped into separate containers
of 10.0 grams of water at room temperature. When the systems come to equilibrium, the container with the
silver will be at the higher temperature.

Question 1 options:

	True
	False

Answer 1

specific heat capacity of silver = 0.240 J/g.oC

specific heat capacity of copper = 0.385 J/g.oC

specific heat capacity of water = 4.184 J/g.oC

Room temperature is 27 oC

when silver and water are mixed

heat lost by silver = heat gained by water

1.0*0.240*(100-T) = 10.0*4.184*(T-27)

24 - 0.24*T = 41.84*T - 1129.7

T = 27.4 oC

when copper and water are mixed

heat lost by silver = heat gained by water

1.0*0.385*(100-T) = 10.0*4.184*(T-27)

38.5 - 0.385*T = 41.84*T - 1129.7

T = 27.7 oC

We can see that container with copper is at higher temperature

Answer: False