Skip to main content
Ch.10 - Gases
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 15th EditionCh.10 - Gases문제 118c
10장, 문제 118c

A 6.53-g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.72 L of carbon dioxide gas at 28°C and 743 torr pressure. c. Assuming that the reactions are complete, calculate the percentage by mass of magnesium carbonate in the mixture.

검증된 단계별 안내
1
Convert the volume of CO₂ gas from liters to moles using the ideal gas law: PV = nRT. Remember to convert temperature to Kelvin and pressure to atmospheres.
Write the balanced chemical equations for the reactions of magnesium carbonate and calcium carbonate with hydrochloric acid, noting that both produce CO₂ gas.
Determine the total moles of CO₂ produced from the reactions using the ideal gas law calculation.
Set up a system of equations based on the stoichiometry of the reactions to relate the moles of CO₂ to the moles of magnesium carbonate and calcium carbonate in the mixture.
Solve the system of equations to find the mass of magnesium carbonate, then calculate the percentage by mass of magnesium carbonate in the original mixture.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
13m

주요 개념

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

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this question, stoichiometry will help relate the amount of carbon dioxide produced to the amounts of magnesium carbonate and calcium carbonate in the mixture.
추천 영상:
가이드 코스
01:16
Stoichiometry Concept

Ideal Gas Law

The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. This law is essential for calculating the moles of carbon dioxide produced in the reaction, which is necessary for determining the composition of the original mixture.
추천 영상:
가이드 코스
01:15
Ideal Gas Law Formula

Percentage by Mass

Percentage by mass is a way to express the concentration of a component in a mixture. It is calculated by dividing the mass of the component by the total mass of the mixture and multiplying by 100. In this problem, calculating the percentage by mass of magnesium carbonate requires determining its mass from the stoichiometric calculations and comparing it to the total mass of the sample.
추천 영상:
가이드 코스
00:38
Mass Percent Calculation
관련 실천
교과서 질문

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I2(s) + 5 F2(g) → 2 IF5(g) A 5.00-L flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C.  (c) Draw the Lewis structure of IF5.

992
views
교과서 질문

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I2(s) + 5 F2(g) → 2 IF5(g) A 5.00-L flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (d) What is the total mass of reactants and products in the flask?

1483
views
교과서 질문

Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I2(s) + 5 F2(g) → 2 IF5(g) A 5.00-L flask containing 10.0 g of I2 is charged with 10.0 g of F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 °C. (a) What is the partial pressure of IF5 in the flask?

982
views