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13 Question (2 points) U LAUNCH TUTORIAL LESSON COAST Tutorial Problem A reaction vessel contains 12.90 g of CO and 12.90 g of Oz. How many grams of CO2 could be produced according to the following reaction? 200+02 2002 v 1st attempt al See Periodic Table SU 9 OF 15 QUESTIONS COMPLETED < 13/15 >

Answer 1

Molar mass of CO = 28g/mol

Molar mass of O2 = 32 g/mol

Molar mass of CO2 = 44 g/mol

Number of mole = mass ÷ molar mass

Therefore

Number of mole of CO = 12.9 ÷ 28 = 0.46 mol

Number of mole of O2 = 12.9 ÷ 32 = 0.403 mol

2CO + O2 ------> 2CO2

According to this to complete the reaction 1 mole of O2 requires 2 mole of CO

Therefore

0.403 mol will requires 2 x 0.403 = 0.806 mol CO but only 0.46 mol is present hence CO is limiting reagent and amount of product form is depend on amount of CO.

Now ,

2 mol CO form 2 mol CO2 hence

0.46 mol CO will form 0.46 mol CO2

Number of mole of CO2 = mass of CO2 ÷ its molar mass

0.46 mol = mass of CO2 ÷ 44g/ mol

Mass of CO2 = 0.46 mol × 44 g/mol

Mass of CO2 = 20.24 gram