How many moles of \ce{CO2}COX
2


will be produced from 72.0 \text{ g}72.0 g72, point, 0, start text, space, g, end text of \ce{CH4}CHX
4


assuming \ce{O2}OX
2


is available in excess?

4.5 moles of carbon dioxide

Explanation:

Given parameters:

Mass of CH₄   = 72g

Unknown:

number of moles of CO₂ produced  = ?

Solution:

To solve this problem, let us write the reaction equation first;

            CH₄     +    2O₂     →    CO₂    +   2H₂O

Now we know that O₂ is in excess and CH₄ is the limiting reactant that will determine the extent of the reaction.

Let us find the number of moles of   CH₄ ;

                Number of moles  =

                                  molar mass of  CH₄ = 12 + 4  = 16g/mol

              Number of moles  =   = 4.5moles

From the reaction equation;

                     1 mole of methane produced 1 mole of carbon dioxide

       4.5 moles of methane will produce 4.5 moles of carbon dioxide

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.

answerlinnaeus;