Question

A 26.4 g sample of aluminum at 100.6 °C is added to 100.4 g of water at 22.0 °C in a constant pressure calorimeter. What is the final temperature of the water in °C? The specific heat capacity of aluminum is 0.903 J/g°C .

Answer 1

Answer: The final temperature of water is 27.82°C

Step-by-step 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.

`Heat_{\text{absorbed}}=Heat_{\text{released}}`

The equation used to calculate heat released or absorbed follows:

`Q=m* c* \Delta T=m* c* (T_(final)-T_(initial))`

`m_1* c_1* (T_(final)-T_1)=-[m_2* c_2* (T_(final)-T_2)]` ......(1)

where,

q = heat absorbed or released

`m_1` = mass of aluminium = 26.4 g

`m_2` = mass of water = 100.4 g

`T_(final)` = final temperature = ?°C

`T_1` = initial temperature of aluminium = 100.6°C

`T_2` = initial temperature of water = 22.0°C

`c_1` = specific heat of aluminium = 0.903 J/g°C

`c_2` = specific heat of water= 4.186 J/g°C

Putting values in equation 1, we get:

`26.4* 0.903* (T_(final)-100.6)=-[100.6* 4.186* (T_(final)-23.7)]`

`T_(final)=27.82^oC`

Hence, the final temperature of water is 27.82°C