Question

A sample of copper is heated to 122.0 C and then placed in a container of 500 g of water at 25.3 °C. The final temperature of the water and copper is 29.7 °C. What is the mass of the copper assuming that all the heat lost by the copper is gained by the water? The specific heat capacity of copper is 0.20 J/°C g.

Answer 1

500.542

Step-by-step explanation:

edge

Answer 2

Mass of copper is 500.542 g.

Step-by-step explanation:

Initial temperature of copper =
`122^(0)`C

specific heat capacity of copper = 0.20 J/°C g

Mass of water = 500 g

Initial temperature of water =
`25.3^(0)`C

Specific heat capacity of water = 4.2 J/°C g

Final temperature of water and copper =
`29.7^(0)` C

Heat loss by copper = Heat gained by water

`m_(c)`
`c_(c)`Δ
`T_(c)` =
`m_(w)`
`c_(w)`Δ
`T_(w)`

`m_(c)` x 0.2 x (122 - 29.7) = 500 x 4.2 x (29.7 - 25.3)

`m_(c)` x 0.2 x 92.3 = 500 x 4.2 x 4.4

`m_(c)` x 18.46 = 9240

`m_(c)` =
`(9240)/(18.46)`

= 500.5417

mass of copper is 500.542 g.