1. The gas left in a used aerosol can is at a pressure of 1 atm at 27( if this can is thrown into a fire, what is the internal pressure of the gas when its temperature reaches 927(C?

4atm

Explanation:

Step 1:

Data obtained from the question. This include the following:

Initial pressure (P1) = 1atm

Initial temperature (T1) = 27°C

Final temperature (T2) = 927°C

Final pressure (P2) =..?

Step 2:

Conversion of celsius temperature to Kelvin temperature.

This can obtained as follow:

T(K) = T (°C) + 273

Initial temperature (T1) = 27°C

Initial temperature (T1) = 27°C + 273 = 300K

Final temperature (T2) = 927°C

Final temperature (T2) = 927°C + 273 = 1200K

Step 3:

Determination of the new pressure of the gas.

This can be obtained as follow:

P1/T1 = P2/T2

Initial pressure (P1) = 1atm

Initial temperature (T1) = 300K

Final temperature (T2) = 1200K

Final pressure (P2) =..?

1/300 = P2 /1200

Cross multiply to express in linear form

300 x P2 = 1 x 1200

Divide both side by 300

P2 = 1200/300

P2 = 4atm

Therefore, the new pressure of the gas is 4atm.

- aluminum and copper chloride.

- the chloride ion to separate the aluminum from the oxygen so that the aluminum can react with the copper ions (and the water molecules).