X litres of carbon monoxide is present at STP. It is completely oxidized to CO2. The volume of CO2 formed is 11.207L at STP. What is the value of X in litres?

11.207 L

Explanation:

In first place, we need to state the reaction:

2CO(g) + O₂(g) →  2CO₂(g)

Ratio is 2:2, so 2 moles of CO can produce 2 moles of CO₂

At STP conditions, 1 mol of any gas occupy 22.4 L. Therefore if our volume is 11.207 L we are having 0.500 moles of gas. Let's verify with the Ideal Gases Law:

1 atm . 11.207 L = n . 0.082 . 273.15K

1 atm . 11.207 L / 0.082 . 273.15K = 0.500 moles.

As ratio is 2:2, 0.500 moles of CO₂ came from 0.500 moles of CO

So the volume in STP, must be the same!

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.