A3.35 gram sample of an unknown gas is found to occupy a volume of 1.64 l at a pressure of 706 mmhg and a temperature of 59 °c. assume ideal behavior. the molar mass of the unknown gas is g/mol.

 The molar mass of the unknown gas is 59.8 g/mol

Explanation:

According to the ideal gas equation:-

P= Pressure of the gas = 706 mmHg = 0.93 atm    (760mmHg=1atm)

V= Volume of the gas = 1.64 L

T= Temperature of the gas = 59°C=(59+273)K=332 K   (0°C = 273 K)

R= Value of gas constant = 0.0821 Latm\K mol

To calculate the moles, we use the equation:

Thus the molar mass of the unknown gas is 59.8 g/mol

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.