A student carried heated a 25.00 g piece of aluminum to a temperature of 100°C, and placed it in 100.00 g of water, initially at a temperature of 10.0°C. Determine the final temperature of the system (aluminum and water)

cH2OB4.18J/gc

c Aluminum .900 j/g c

The final temperature of the system is 14.60°C

Explanation:

When metal is dipped in water, the amount of heat released by metal will be equal to the amount of heat absorbed by water.

The equation used to calculate heat released or absorbed follows:

     ......(1)

where,

q = heat absorbed or released

= mass of aluminium = 25.00 g

= mass of water = 100 g

= final temperature = ?°C

= initial temperature of aluminium = 100°C

= initial temperature of water = 10°C

= specific heat of aluminium = 0.900 J/g°C

= specific heat of water= 4.18 J/g°C

Putting values in equation 1, we get:

Hence, the final temperature of the system is 14.60°C

14 days is the half-life of phosphorus-32