Which gas law would you use for the following problem: What pressure is required to hold 8.0 moles of oxygen gas in an 8.0 L container at a temperature of 80 degrees Celsius? Boyle’s Law

Charles’ Law

Combined Gas Law

Ideal Gas Law

Ideal Gas Law ( PV = nRT)

Explanation:

Using the Ideal Gas Law, we have; PV = nRT

Where P= Pressure = ?

            V= Volume = 8.0 L

            n =  moles = 8.0

            R =  Gas constant = 0.0821 L.atm/mol/K

            T =  80° c + 273 =  353.15K

Therefore Pressure would be;  P = nRT/ V =  8 x 0.0821 x 353.15 / 8 = 28.9atm

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.