To determine the molar mass of an unknown gas, its effusion time was compared to Oscon gas, which has a molar mass of 42.005g - mol1. A sample of Oscon was found to effuse from a container in 41.71 Part A seconds. The same amount of the unknown gas requires 91.76 seconds. Rateoscon Rateunknown Determine the ratio Hint the times are not the individual rates themselves. Rates are an amount per time. Express your answer using four significant figures. ? RateOncon Ratenknown

To determine the molar mass of an unknown gas, its effusion time was compared to Oscon gas, which has a molar mass of 42.005g - mol1. A sample of Oscon was found to effuse from a container in 41.71 Part A seconds. The same amount of the unknown gas requires 91.76 seconds. Rateoscon Rateunknown Determine the ratio Hint the times are not the individual rates themselves. Rates are an amount per time. Express your answer using four significant figures. ? RateOncon Ratenknown

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5.105PAE: 105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so...

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When two cotton plugs. one moistened with ammonia and the other with hydrochloric acid, are simultaneously inserted into opposite ends of a glass tube that is 87.0 cm long, a white 1111g of NH4Cl forms where gaseous NH3 and gaseous HC1 first come into contact. NH3(g)+HCl(g)NH4Cl(s) At approximately what distance from the ammonia moistened plug does this occur? (Hint: Calculate the rates of diffusion for both NH3 and HCI, and find out how much faster NH3 diffuses than HCI.)
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
Carbon dioxide, CO2, was shown lo effuse through a porous plate at the rate of 0.033 mol/min. The same quantity of an unknown gas, 0.033 moles, is found to effuse through the same porous barrier in 104 seconds. Calculate the molar mass of the unknown gas.
Xenon and fluorine will react to form binary compounds when a mixture of these two gases is heated to 400C in a nickel reaction vessel. A 100.0-mL nickel container is filled with xenon and fluorine, giving partial pressures of 1.24 atm and 10.10 atm, respectively, at a temperature of 25C. The reaction vessel is heated to 400C to cause a reaction to occur and then cooled to a temperature at which F2 is a gas and the xenon fluoride compound produced is a nonvolatile solid. The remaining F2 gas is transferred to another 100.0-mL nickel container, where the pressure of F2 at 25C is 7.62 atm. Assuming all of the xenon has reacted, what is the formula of the product?
At elevated temperatures, sodium chlorate decomposes to produce sodium chloride and oxygen gas. A 0.8765-g sample of impure sodium chlorate was heated until the production of oxygen gas ceased. The oxygen gas collected over water occupied 57.2 mL at a temperature of 22C and a pressure of 734 torr. Calculate the mass percent of NaClO3 in the original sample. (At 22C the vapor pressure of water is 19.8 torr.)
105 The decomposition of mercury(II) thiocyanate produces an odd brown snake-like mass that is so unusual the process was once used in fireworks displays. There are actually several reactions that take place when the solid Hg(SCN)2 is ignited: 2Hg(SCN)2(s)2HgS(s)+CS2(s)+C3N4(s)CS2(s)+3O2(g)CO2(g)+2SO2(g)2C3N4(s)3(CN)2(g)+N2(g)HgS(s)+O2(g)Hg(l)+SO2(g) A 42.4-g sample of Hg(SCN)2 is placed into a 2.4-L vessel at 21°C. The vessel also contains air at a pressure of 758 torr. The container is sealed and the mixture is ignited, causing the reaction sequence above to occur. Once the reaction is complete, the container is cooled back to the original temperature of 21°C. (a) Without doing numerical calculations, predict whether the final pressure in the vessel will be greater than, less than, or equal to the initial pressure. Explain your answer. (b) Calculate the final pressure and compare your result with your prediction. (Assume that the mole fraction of O2 in air is 0.21.)
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
38 For a gas sample whose total pressure is 740 torr, what are the partial pressures if the gas present consists of 1.3 mol of N2, 0.33 mol of O2, and 0.061 moI of Ar?