Acontainer is filled with hydrogen gas. it has a volume of 4 liters and a pressure of 2 atm. if the pressure of the container is increased to 6 atm without removing any of the gas or changing the temperature, what will the new volume be

1.33 L.

Explanation:

where, P is the pressure of the gas in atm.

V is the volume of the gas in L.

n is the no. of moles of the gas in mol.

R  is the general gas constant,

T is the temperature of the gas in K.

(P₁V₁) = (P₂V₂)

Knowing that:

V₁  =  4.0 L, P₁ = 2.0 atm,

V₂  =  ??? L, P₂ = 6.0 atm.

(P ₁V₁) = (P₂V₂)

∴ V₂ = P ₁V₁/P₂ = (2.0 atm)(4.0 L)/(6.0 atm) = 1.33 L.

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

58750.08068 is the answer i think