Chemistry chemical reactions

Question

A reaction vessel contains 7.10 g of CO and 7.10 g of O₂. How many grams of CO₂ could be produced according to the following reaction?

2CO+O2​2CO2​

Answer 1

2CO + O₂ ==> 2CO₂ .. balanced equation

To answer this problem, we will first find the moles of CO and moles of O₂ present. From the mol ratio of the balanced equation, we'll determine which reactant is limiting. Using the moles of the limiting reactant, we'll find the moles of CO₂ produced and finally convert that to grams of CO₂ produced.

Info needed:

molar mass CO = 28.01 g / mol

molar mass O₂ = 32.0 g / mol

molar mass CO₂ = 44.0 g / mol

moles CO present = 7.10 g CO x 1 mol CO / 28.01 g = 0.253 mols CO

moles O₂ present = 7.10 g O₂ x 1 mol O₂ / 32.0 g = 0.222 mols O₂

Since the balanced equation tells us that we need 2 mols CO for every 1 mol O₂, CO will be limiting because we don't have twice as many moles as O₂.

Moles of CO₂ produced = 0.253 mols CO x 2 mols CO₂ / 2 mols CO = 0.253 mols CO₂

Mass of CO₂ = 0.253 mols CO₂ x 44.0 g CO₂ / mol = 11.1 g CO₂ (3 sig. figs.)