An empty Erlenmeyer flask that weighs 93.667g has a quantity of liquid vaporized in it at 93.2°C and a pressure of 960. torr. The mass of the cooled flask is 94.397g. When the flask is filled with water, the mass of the flask and water is 318.667g. (a). Determine the molecular weight of the unknown liquid. g/mol *Write answer in decimal form to one decimal place, NO units in answer** (b). Given the following compounds: Liquid Molecular Weight (g/mole) Pentane 72.2 Heptane Diethyl ether 100.2 74.1 Cyclopropane 42.1 Pentanol 88.2 Octanol 130.2 What is the identity of the unknown liquid?

An empty Erlenmeyer flask that weighs 93.667g has a quantity of liquid vaporized in it at 93.2°C and a pressure of 960. torr. The mass of the cooled flask is 94.397g. When the flask is filled with water, the mass of the flask and water is 318.667g. (a). Determine the molecular weight of the unknown liquid. g/mol *Write answer in decimal form to one decimal place, NO units in answer** (b). Given the following compounds: Liquid Molecular Weight (g/mole) Pentane 72.2 Heptane Diethyl ether 100.2 74.1 Cyclopropane 42.1 Pentanol 88.2 Octanol 130.2 What is the identity of the unknown liquid?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

In the Haber reaction, patented by German chemist Fritz Haber in 1908, dinitrogen gas combines with dihydrogen gas to produce gaseous ammonia. This reaction is now the first step taken to make most of the world's fertilizer. Suppose a chemical engineer studying a new catalyst for the Haber reaction finds that 715. liters per second of dinitrogen are consumed when the reaction is run at 153. °C and the dinitrogen is supplied at 0.18 atm. Calculate the rate at which ammonia is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. kg S Continue dallall 80 x10 X 802 S ? JUN 27 © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A O Submit Assi tv .
A flask contains a mixture of two gases: NO2 and Ne. The flask holds 0.519 mol of NO2 and an unknown amount of Ne. If the partial pressure of Ne is 0.43 bar and the total pressure in the flask is 0.83 bar, calculate the mass of Ne in the flask (in g). TIP: You don't need the volume of the flask nor the temperature to solve this problem. Express answer in 2 significant figures.
Nitrous oxide (N₂O), also known as laughing gas, has uses in surgery and dentistry as an anesthetic. The molecular weight of the nitrous oxide cylinder is 44.013 g/mol. Assuming standard temperature and pressure, what would be the volume, in L, of a cylinder containing 4.23 kg of nitrous oxide?
Q1. An organic chemist isolates a colourless liquid from a petroleum sample. She places the liquid in a flask and puts the flask in a boiling water bath, which vaporizes the liquid and fills the flask with gas. She closes the flask, reweighs it, and obtains the following data: Volume of flask (V) = 213 mL T=100°C P=754 torr (760 torr in 1 atmosphere) Mass of flask+gas = 78.416g Mass of empty flask = 77.834g Calculate the molar mass of the liquid, carefully converting to appropriate units, where necessary. (Note: Gas constant; R = 0.082057 L.atm.K-¹.mol-¹)
Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas wells. In the first step of this synthesis, called the Claus process, hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water. Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 421. liters per second of dioxygen are consumed when the reaction is run at 280. °C and the dioxygen is supplied at 0.35 atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Be sure your answer has the correct number of significant digits. 00 S X 6 000 Ar B
A colleague of yours takes a bunch of pressure readings while you are gone. You return to realize that he has invented a new unit: his body mass of 180lb per 1mile?. He calls this unit Bob per Bob's Block. 1mile = 63360 inches. What is the pressure of 9 Bobs per Bob's block in a real unit of pressure, pounds per square inch (PSI)? Use just one sig fig in your answer: x10^ PSI
Solid ammonium chloride, NH4Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen chloride, HCl. NH3(g)+HCl(g)⟶NH4Cl(s) A 3.52 g sample of NH3 gas and a 3.52 g sample of HCl gas are mixed in a 2.00 L flask at 25 ∘C. Identify the limiting reagent. NH4Cl HCl NH3 How many grams of NH4Cl will be formed by this reaction? What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH4Cl produced by the reaction. ?=
A 2.61 gram sample of a solid mixture contains NaClO3 as well as unreactive material. When heated, only the NaClO3 in the mixture decomposes to produce 992 milliliters of O2 gas at 225◦C and 772 mmHg according to the unbalanced equation NaClO3(s) −→ NaCl(s) + O2(g). What is the percent by mass of NaClO3 in the mixture?
A COVID-19 patient is in hospital receiving supportive oxygen therapy for respiratory distress. The patient is receiving a mixture of air which contains 325 mmHg of Nitrogen, 223 mmg of Oxygen, 20 mmHg of Argon, and 15 mmHg of Carbon Dioxide. What is the FO2 for the air that the patient is breathing? (Express your answer to 3 decimal places)
At a certain temperature, 0.361 mol CH40.361 mol CH4 and 0.667 mol H2O0.667 mol H2O is placed in a 2.50 L2.50 L container. CH4(g)+2H2O(g)↽−−⇀CO2(g)+4H2(g)CH4⁢(g)+2⁢H2O(g)⁢↽−−⇀⁢CO2⁢(g)+4⁢H2⁡(g) At equilibrium, 7.88 g CO27.88 g CO2 is present. Calculate ?cKc.
Most of the sulfur used in the United States is chemically synthesized from hydrogen sulfide gas recovered from natural gas wells. In the first step of this synthesis, called the Claus process, hydrogen sulfide gas is reacted with dioxygen gas to produce gaseous sulfur dioxide and water. Suppose a chemical engineer studying a new catalyst for the Claus reaction finds that 329. liters per second of dioxygen are consumed when the reaction is run at 178.°C and the dioxygen is supplied at 0.65atm. Calculate the rate at which sulfur dioxide is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits. =___kg/s