From this combustion equation, 2CH22 + 3102 - 22H,0 + 2000, calculate the liters of
carbon dioxide produced when 16.9 grams of CH are combusted

Answer : The volume of produced are, 26.7 liters.

Explanation :

First we have to calculate the moles of

Now we have to calculate the moles of .

The given combustion reaction is:

From the balanced chemical reaction we conclude that,

As, 2 moles of react to give 20 moles of

So, 0.119 moles of react to give moles of

Now we have to calculate the volume of produced.

As we know that, 1 mole of gas occupies 22.4 L volume of gas.

As, 1 mole of gas occupies 22.4 L volume of gas.

So, 1.19 mole of gas occupies 1.19 × 22.4 L = 26.7 L volume of gas.

Therefore, the volume of produced are, 26.7 liters.

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.