Skip to main content
Ch.5 - Gases
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.5 - Gases문제 80
5장, 문제 80

Carbon monoxide gas reacts with hydrogen gas to form methanol. CO(g) + 2 H2(g) → CH3OH(g) A 1.50-L reaction vessel, initially at 305 K, contains carbon monoxide gas at a partial pressure of 232 mmHg and hydrogen gas at a partial pressure of 397 mmHg. Identify the limiting reactant. Determine the theoretical yield of methanol in grams.

검증된 단계별 안내
1
Write the balanced chemical equation for the reaction: \( \text{CO(g)} + 2 \text{H}_2\text{(g)} \rightarrow \text{CH}_3\text{OH(g)} \).
Use the ideal gas law \( PV = nRT \) to calculate the number of moles of CO and \( \text{H}_2 \) in the reaction vessel. Assume \( R = 0.0821 \text{ L atm mol}^{-1} \text{ K}^{-1} \) and convert pressures from mmHg to atm.
Determine the limiting reactant by comparing the mole ratio of CO to \( \text{H}_2 \) with the stoichiometric ratio from the balanced equation.
Calculate the theoretical yield of methanol by using the moles of the limiting reactant and the stoichiometry of the reaction to find the moles of \( \text{CH}_3\text{OH} \) produced.
Convert the moles of \( \text{CH}_3\text{OH} \) to grams using its molar mass (32.04 g/mol).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

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 it, one must compare the mole ratios of the reactants based on the balanced chemical equation. The reactant that produces the least amount of product is the limiting reactant.
추천 영상:
가이드 코스
01:30
Limiting Reagent Concept

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. This concept is crucial for calculating the number of moles of each reactant present in the reaction vessel.
추천 영상:
가이드 코스
00:48
Partial Pressure Calculation

Theoretical Yield

The theoretical yield is the maximum amount of product that can be generated from a given amount of reactants, assuming complete conversion and no losses. It is calculated using stoichiometry based on the limiting reactant. The theoretical yield is typically expressed in grams and is essential for evaluating the efficiency of a chemical reaction.
추천 영상:
가이드 코스
03:09
Percent Yield in Reactions
관련 실천
교과서 질문

A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. a. Which of the two gases exerts the greater partial pressure?

1666
views
교과서 질문

A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. b. The molecules or atoms of which gas have the greater average velocity? d. If a small hole were opened in the flask, which gas effuses more quickly?

교과서 질문

Ozone is depleted in the stratosphere by chlorine from CF3Cl according to this set of equations:

CF3Cl + UV light → CF3 + Cl

Cl + O3 → ClO + O2

O3 + UV light → O2 + O

ClO + O → Cl + O2

What total volume of ozone at a pressure of 25.0 mmHg and a temperature of 225 K is destroyed when all of the chlorine from 15.0 g of CF3Cl goes through 10 cycles of the given reactions?

1494
views
교과서 질문

Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: CH4(g) + H2O(g) → CO(g) + 3 H2(g) In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?

5161
views
교과서 질문

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.

5162
views
1
rank
교과서 질문

Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure. a. Do the atoms in the helium sample have the same average kinetic energy as the atoms in the argon sample?

1350
views