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Questions and Answers
What is the molar mass of (NH2)2CO?
In the reaction to produce (NH2)2CO, which compound is the limiting reagent?
How many moles of (NH2)2CO can be produced from 1142 g of CO2 in the reaction?
What is the mass of (NH2)2CO produced from 18.71 moles of (NH2)2CO?
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From the given data, what can be said about the role of NH3 in the reaction?
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If more NH3 was added to the reaction, what would be the impact on the production of (NH2)2CO?
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What does the molar ratio between NH3 and (NH2)2CO tell us about the reaction?
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Which compound plays a crucial role in converting moles of CO2 to moles of (NH2)2CO?
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'Mole fraction' refers to:
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Study Notes
Limiting Reagent
- The limiting reagent is the reactant that yields the smaller amount of the product.
- It is the reactant that gets consumed first and limits the amount of product formed.
Calculating the Limiting Reagent
- To determine the limiting reagent, calculate the number of moles of product obtainable from each reactant.
- The reactant that produces the smaller amount of product is the limiting reagent.
Example: NO2 Formation
- 8 moles of NO yields 2 moles of NO2.
- 7 moles of O2 yields 14 moles of NO2.
- Therefore, NO is the limiting reagent, and O2 is the excess reagent.
Problem: (NH2)2CO Formation
- The balanced chemical equation is CO2(g) + 2NH3(g) → (NH2)2CO(aq) + H2O(l).
- 637.2 g of NH3 reacts with 1142 g of CO2.
- NH3 is the limiting reagent, producing 18.71 moles of (NH2)2CO.
- The mass of (NH2)2CO formed is 1124 g.
Excess Reagent
- The excess reagent is the reactant that is left over after the reaction is complete.
- In this case, the excess reagent is CO2.
- The mass of excess CO2 is the initial mass minus the mass that reacted.
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Description
Test your knowledge on determining the limiting reagent in a chemical reaction by calculating the moles of product obtainable from given initial quantities of reactants. Understand how to identify which reactant limits the amount of product formed.
