Find the mass of benzene (C6H6) required to produce 2.66 g of carbon dioxide gas from the reaction described by the following equation: 2C6H6 + 15O2 → 6H2O + 12CO2

Mass of benzene required = 0.78 g

Explanation:

Given data:

Mass of CO₂ produced = 2.66 g

Mass of benzene required = ?

Solution:

Chemical equation:

2C₆H₆ + 15O₂       →    6H₂O + 12CO₂

Number of moles of CO₂:

Number of moles = mass/molar mass

Number of moles = 2.66 g/ 44 g/mol

Number of moles = 0.06 mol

Now we will compare the moles of CO₂ with C₆H₆.

                        CO₂       :        C₆H₆

                            12        :          2

                          0.06      :        2/12×0.06=0.01 mol

Mass of benzene required:

Mass = number of moles × molar mass

Mass = 0.01 mol × 78.11 g/mol

Mass = 0.78 g

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.