A scientist looking to remove oxygen from above a liquid sample pumps nitrogen into a sealed compartment to displace the oxygen, then places his liquid sample into the compartment. If the nitrogen pressure (partial pressure) was 1.8 atm, what would be the concentration of dissolved nitrogen gas if the Henry’s Law constant for nitrogen gas was 6.8 × 10-4 M atm-1 at this temperature?

1.2 × 10^-3 M

Explanation:

Henry's law law states that; once the temperature is constant, the amount of a given mass of gas that is dissolved in a particular type and volume of solvent is directly proportional to the partial pressure of that gas in equilibrium with the solvent.

From Henry's law;

Cg= K × Pg

Where;

Cg = concentration of gas

K= constant of Henry's law

Pg= partial pressure of the gas

Cg= 6.8 × 10^-4 M atm^-1 × 1.8 atm

Cg = 1.2 × 10^-3 M

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.