When 0.110 mol of carbon is burned in a closed vessel with 9.71 g of oxygen,...

When 0.110 mol of carbon is burned in a closed vessel with 9.71 g of oxygen, how many grams of carbon dioxide can form?

Which reactant is in excess, and how many grams of it remain after the reaction?

Expert Solution

Lets calculate the moles of oxygen first:

molar mass of oxygen = 32 g/mol

moles = mass / molar mass = 9.71 g/ 32g/mol = 0.3034 mol

now write the reaction equation:

C + O₂ → CO₂

stoichiometric conversion factor for O₂ consumed = 1 mol C / 1 mol O₂

0.3034 mol O₂ needs = 1 mol C / 1 mol O₂ x 0.3034 mol O₂

= 0.3034 mol C

but we have only 0.110 mol C and hence it is limiting reactant and O₂ is in excess

now the conversion will be based on limiting reactant only as the reaction will stop as soon as limiting reactant is over:

0.11 mol C needs 0.11 mol O₂

remaining O₂ = 0.3034 mol - 0.11 mol = 0.1934 mol

= 0.1934 mol x 32g/mol = 6.19 g will be left after reaction completion

please upvote thanks!

queen_honey_blossom answered 2 years ago

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