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 101
5장, 문제 101

Consider the reaction: 2 NiO(s) → 2 Ni(s) + O2(g). If O2 is collected over water at 40.0 °C and a total pressure of 745 mmHg, what volume of gas is collected for the complete reaction of 24.78 g of NiO?

검증된 단계별 안내
1
Calculate the molar mass of NiO by adding the atomic masses of Ni and O.
Determine the number of moles of NiO by dividing the given mass (24.78 g) by the molar mass of NiO.
Use the stoichiometry of the balanced chemical equation to find the moles of O2 produced. According to the equation, 2 moles of NiO produce 1 mole of O2.
Use the ideal gas law, PV = nRT, to calculate the volume of O2. First, convert the temperature from Celsius to Kelvin by adding 273.15.
Adjust the total pressure to account for the vapor pressure of water at 40.0 °C, then use the adjusted pressure in the ideal gas law to find the volume of O2.

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 based on the balanced equation. It allows us to determine the amount of product formed or reactant consumed from a given quantity of another substance. In this case, we need to use the molar ratios from the balanced equation to find out how much O2 is produced from the decomposition of NiO.
추천 영상:
가이드 코스
01:16
Stoichiometry Concept

Gas Laws

Gas laws describe the behavior of gases in relation to pressure, volume, and temperature. The Ideal Gas Law (PV=nRT) is particularly useful for calculating the volume of gas produced under specific conditions. In this scenario, we will apply the gas laws to determine the volume of O2 collected, taking into account the total pressure and the vapor pressure of water at 40.0 °C.
추천 영상:
가이드 코스
01:43
Combined Gas Law

Vapor Pressure of Water

The vapor pressure of water is the pressure exerted by water vapor in equilibrium with its liquid at a given temperature. At 40.0 °C, the vapor pressure of water must be subtracted from the total pressure to find the partial pressure of the O2 gas collected. This adjustment is crucial for accurately calculating the volume of O2 produced in the reaction.
추천 영상:
가이드 코스
02:40
Raoult's Law and Vapor Pressure
관련 실천
교과서 질문

A gaseous hydrogen- and carbon-containing compound is decomposed and found to contain 85.63% C and 14.37% H by mass. The mass of 258 mL of the gas, measured at STP, was 0.646 g. What is the molecular formula of the compound?

2574
views
3
rank
교과서 질문

Consider the reaction: 2 Ag2O(s) → 4 Ag(s) + O2(g) If this reaction produces 15.8 g of Ag(s), what total volume of gas can be collected over water at a temperature of 25 °C and a total pressure of 752 mmHg?

407
views
교과서 질문

Consider the reaction:

2 SO2(g) + O2(g) → 2 SO3(g)

a. If 285.5 mL of SO2 reacts with 158.9 mL of O2 (both measured at 315 K and 50.0 mmHg), what is the limiting reactant and the theoretical yield of SO3?

1301
views
교과서 질문

A gaseous hydrogen- and carbon-containing compound is decomposed and found to contain 82.66% carbon and 17.34% hydrogen by mass. The mass of 158 mL of the gas, measured at 556 mmHg and 25 °C, was 0.275 g. What is the molecular formula of the compound?

1365
views