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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 80a
Capitolo 3, Problema 80a

One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (a) Which is the limiting reactant?

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Step 1: Write down the balanced chemical equation. In this case, it is already given: 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
Step 2: Calculate the number of moles of each reactant. The molar mass of NH3 is approximately 17 g/mol and the molar mass of O2 is approximately 32 g/mol. So, divide the given mass of each reactant by its molar mass to find the number of moles.
Step 3: Determine the stoichiometric ratio from the balanced chemical equation. In this case, it is 4 moles of NH3 to 5 moles of O2.
Step 4: Compare the ratio of the number of moles of each reactant to the stoichiometric ratio. The reactant that is less than or equal to its stoichiometric ratio is the limiting reactant.
Step 5: If it's not clear which reactant is the limiting one, calculate the amount of product that each reactant could produce. The reactant that produces the least amount of product is the limiting reactant.

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Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows chemists to determine the proportions of substances involved in a reaction, which is essential for identifying limiting reactants. In this case, stoichiometry will help calculate how much NH3 and O2 are needed to produce NO and H2O.
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Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for predicting the yield of products. In this experiment, comparing the mole ratios of NH3 and O2 will reveal which reactant limits the formation of NO.
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Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is essential for converting between grams and moles, which is necessary for stoichiometric calculations. In this question, calculating the molar masses of NH3 and O2 will allow for the determination of the number of moles present, facilitating the identification of the limiting reactant.
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One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.

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One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: 4 NH31g2 + 5 O21g2¡4 NO1g2 + 6 H2O1g2 In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2. (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed?

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