How many moles of oxygen (O2) are present in 33.6 L of the gas at 1 atm and 0°C?
1.5
O2
22.4
0 32
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The answer is 1.5 moles.

Explanation:

An ideal gas is a theoretical gas that is considered to be composed of point particles that move randomly and do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law:

P * V = n * R * T

where n is the number of moles and R is the molar constant of the gases.

In this case:

Replacing:

1 atm*33.6 L= n* 0.082 *273 °K

Solving:

n= 1.5 moles

So, the answer is 1.5 moles.

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.