
Concept explainers
Interpretation:
The mass of CO2 and CO formed when 5.00 g of carbon is burned under excess and restricted supply of oxygen needs to be deduced from the given reactions.
Concept Introduction:
- A
chemical reaction is represented as a chemical equation with the reactants and the products on the left and right side of the reaction arrow respectively.
- The coefficient of a balanced chemical equation, i.e., the stoichiometry gives the number of reactants and products involved in the reaction.
- Chemical equations can therefore be used to determine the amount of products formed from a known quantity of reactants.

Answer to Problem 19A
Mass of CO = 18.33 g
Mass of CO2 = 11.67 g
Explanation of Solution
a) Reaction in excess oxygen:
The given reaction is:
Step 1: Calculate the moles of C present:
Mass of C present = 5.0 g
Atomic weight of C = 12 g/mole
Step 2: Calculate the moles of CO2 formed:
Based on the reaction stoichiometry:
1 mole of Creacts to form 1 mole of CO2
Therefore, 0.4167 moles of C would produce 0.4167 moles of CO2
Step 3: Calculate the mass of CO2 formed:
Moles of CO2 = 0.4167
Molecular weight of CO2 = 44 g/mol
b) Reaction in restricted oxygen:
The given reaction is:
Step 1: Calculate the moles of C present:
Mass of C present = 5.0 g
Atomic weight of C = 12 g/mole
Step 2: Calculate the moles of CO formed:
Based on the reaction stoichiometry:
2 moles of C reacts to form 2 mole of CO
Therefore, 0.4167 moles of C would produce:
Step 3: Calculate the mass of CO formed:
Moles of CO = 0.4167
Molecular weight of CO = 28 g/mol
Therefore, 18.33 g and 11.67 g of CO and CO2 are produced in excess and restricted supply of oxygen respectively.
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