How many moles of a gas at 104°C would occupy a volume of 6.8
L at a pressure of 270 mm Hg?

0.079mole

Explanation:

From the question given, we obtained the following data:

T = 104°C = 104 + 273 = 377K

V = 6.8L

P = 270 mmHg

Recall: 760mmHg = 1atm

Therefore, 270 mmHg = 270/760 = 0.36atm

R = 0.082atm.L/Kmol

n =?

Using the ideal gas equation:

PV = nRT

We can easily obtain the number of mole as follow:

PV = nRT

n = PV /RT

n = 0.36 x 6.8 / 0.082 x 377

n = 0.079mole

The number of mole of the gas is 0.079mole

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.