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 .

The final temperature of water is 27.82°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 = 26.4 g

= mass of water = 100.4 g

= final temperature = ?°C

= initial temperature of aluminium = 100.6°C

= initial temperature of water = 22.0°C

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

= specific heat of water= 4.186 J/g°C

Putting values in equation 1, we get:

Hence, the final temperature of water is 27.82°C

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

e