Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl₂(g) + 3 F₂(g) → 2 ClF₃(g) A 2.00-L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 729 mmHg. Identify the limiting reactant. Determine the theoretical yield of ClF₃ in grams.

검증된 단계별 안내

Identify the balanced chemical equation: \( \text{Cl}_2(g) + 3 \text{F}_2(g) \rightarrow 2 \text{ClF}_3(g) \).

Convert the partial pressures of \( \text{Cl}_2 \) and \( \text{F}_2 \) to moles using the ideal gas law: \( PV = nRT \). Assume \( R = 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \) and convert pressures from mmHg to atm.

Determine the mole ratio from the balanced equation and compare the mole ratio of available \( \text{Cl}_2 \) and \( \text{F}_2 \) to find the limiting reactant.

Calculate the moles of \( \text{ClF}_3 \) produced using the stoichiometry of the reaction based on the limiting reactant.

Convert the moles of \( \text{ClF}_3 \) to grams using its molar mass (\( \text{ClF}_3 \) molar mass = 92.45 g/mol).

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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. To identify the limiting reactant, one must compare the mole ratios of the reactants based on the balanced chemical equation and the initial amounts available. In this case, the stoichiometry of the reaction Cl2 + 3F2 → 2ClF3 will guide the analysis.

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. In this question, the partial pressures of chlorine and fluorine gases are crucial for calculating the number of moles available for the reaction, which is necessary for determining the limiting reactant.

Theoretical Yield

Theoretical yield is the maximum amount of product that can be produced from a given amount of reactants, assuming complete conversion and no losses. It is calculated using the stoichiometry of the balanced equation and the limiting reactant. Once the limiting reactant is identified, the theoretical yield of ClF3 can be determined by converting moles of the limiting reactant to grams using its molar mass.