If 2.00 moles of nitrogen and 5.50 moles of hydrogen are placed in a reaction vessel and react to form ammonia, what is the theoretical yield of ammonia (NH3)? (LO 3.8) N2(g) + 3 H2(g) --> 2 NH3(g) (a) 31.2 g (b) 62.3 g (c) 93.7 g (d) 34.1

검증된 단계별 안내

Identify the balanced chemical equation: \( N_2(g) + 3 H_2(g) \rightarrow 2 NH_3(g) \).

Determine the limiting reactant by comparing the mole ratio of \( N_2 \) and \( H_2 \) to the coefficients in the balanced equation.

Calculate the moles of \( NH_3 \) produced by the limiting reactant using stoichiometry.

Convert the moles of \( NH_3 \) to grams using the molar mass of \( NH_3 \) (17.03 g/mol).

Compare the calculated mass of \( NH_3 \) to the given options to determine the theoretical yield.

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주요 개념

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Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It allows us to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. In this case, the stoichiometric coefficients from the balanced equation indicate the molar ratios needed to determine the theoretical yield of ammonia.

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. In the given reaction, we need to identify whether nitrogen or hydrogen is the limiting reactant by comparing the mole ratios of the reactants to the coefficients in the balanced equation. This concept is crucial for calculating the theoretical yield of ammonia.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To convert the number of moles of ammonia produced into grams, we must use the molar mass of ammonia (NH3), which is approximately 17.03 g/mol. This conversion is essential for expressing the theoretical yield in grams, as required by the question.