Which gas sample would likely not act like an ideal gas? choose one of the following,

1. a sample of oxgen gas at low pressure

2. a sample of oxygen gas at high temperature

3. a sample of argon gas at high pressure

4. a sample of argon gas at high temperature

5. all gases listed above would behave like ideal gases.

A sample of argon gas at high pressure

Explanation:

A gas behaves more like an ideal gas at higher temperature and lower pressure

A sample of argon gas at high pressure would not act like an ideal gas.

Option C

Explanation:

According to ideal gas law or kinetic theory of gases, the pressure is inversely proportionate to its volume and directly proportionate to temperature and vice versa. So they bind the parameters of pressure of the gas, volume occupied by the gas and temperature of the gas with the moles of the gas in a simple equation,

                                  PV = nRT

where P - the pressure, V - the volume, n - the number of moles, T - the temperature and R - the gas constant. So every ideal gas tend to obey this equation only at certain conditions.

And the conditions where this equation will be applicable is high temperature and low pressure. So among the given options, the sample of argon gas at high pressure will not be acting like an ideal gas as it is at high pressure.

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.

i believe the answer is a.