Imagine you leave a bottle of something toxic to humans open overnight in a sealed laboratory. The levels of solution drastically drop, and you do not know if it is harmful or not with your
knowledge of the ideal gas law, explain how you can determine whether it is safe or not in the
laboratory Use a simple experimental setup to support your argument

Argument: It is not Safe

Further support to the argument is given below.

Explanation:

Solution:

Argument: It is not Safe

First of all, we all know the ideal gas law:

PV = nRT

And the Boyle's Law states that , if the pressure is increased then, volume will decrease. and if the volume is increased then pressure will decrease.

V is inversely proportional to Pressure of the gas.

So, in this case, Let's suppose we have toxic solution of methyl alcohol in the bottle which is tightly closed. It means pressure in the bottle is high, hence the volume is less.

If in this scenario someone, leave the bottle open in the laboratory and as it is given that the level of solution will drastically decrease. It means it is volatile in nature and is converted into gaseous form and we know now that the open bottle has now less pressure. Hence the volume of the gas will be higher and now it can spread to every corner of the laboratory. And it is very dangerous.

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.