A weighed quantity of PCI5(s) is sealed in a 100.0-cm³glass bulb to which a pressure gauge is attached. The bulbis heated to 250°C, and the gauge shows that the pressurein the bulb rises to 0.895 atm. At this temperature, thesolid PCI, is all vaporized and also partially dissociatedinto Cl2(g) and PCI3(g) according to the equationPCI5(g) 2 PCI3(g) + Cl(g)At 250°C, K = 2.15 for this reaction. Assume that thecontents of the bulb are at equilibrium and calculate thepartial pressure of the three different chemical species inthe vessel.

Given: The dissociation of PCl5 takes places as, The volume of the reactor is 100.0 mL The…

Answered: A weighed quantity of PCI5(s) is sealed…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter9: The Gaseous State

Section: Chapter Questions

Problem 33P

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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?
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
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.)
the potetial of the sell Ag/AgI(s)//AgI(aq)/Ag is +0.9509 at 25 degree Celsius. Calculate (i) the soluility product of AgI and (ii) the soluility of AgI.
Consider the following reaction CS2(g) + 3O2(g) → CO2(g) + 2SO2(g) A mixture containing only CS2(g) and excess O2(g) at a total pressure of 100 kPa is placed in a sealed vessel. After the reaction is completed and the vessel is cooled to the initial temperature, the total pressure in the vessel drops to 80 kPa. What is the mole fraction of CO2(g) in the final mixture?
A 10.0 g sample of liquid water is closed in a 1515 mL flask and allowed to reach equilibrium with its vapor at 27ºC. >What is the mass of H2O(g) when equilibrium is established? Data: Pv (H2O, 27ºC) = 26.7 torr.
The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as ??=???P⁢V=n⁢R⁢T where ?P is the pressure, ?V is the volume, ?n is the number of moles of gas, ?R is the ideal gas constant, and ?T is the temperature. Rearrange the equation to solve for ?. then.... At 256 K,256 K, 1.435 mol1.435 mol of an ideal gas occupy a volume of 10.83 L10.83 L and have a pressure of 2.785 atm.2.785 atm. What is the value of the ideal gas constant? R=
Combustible vapor-air mixtures are flammable over a limitedrange of concentrations. The minimum volume % of vapor thatgives a combustible mixture is called the lower flammable limit(LFL). Generally, the LFL is about half the stoichiometric mix-ture, the concentration required for complete combustion of thevapor in air. (a) If oxygen is 20.9 vol % of air, estimate the LFL forn-hexane, C₆H₁₄. (b) What volume (in mL) of n-hexane (d=0.660 g/cm³) is required to produce a flammable mixture of hexane in 1.000 m³of air at STP?
A 500mL sample of O2 gas at 24 degrees Celsius was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2O2, in the presence of a small amount of manganese catalyst by the reaction: 2H2O2(aq) -------> 2H2O(g) + O2(g) The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? Please note that the vapor pressure of water at 24 degrees Celsius is 23 mm Hg.
When hydrogen iodide gas is associated into hydrogen and iodine gases, at temperature of 698.8 K at 1.85 x 10^-2, assess and estimate the weight in grams of hydrogen iodide formed when the gas products formed are heated to 698.8 K in 3.01 liter veassel. Assuming 10.01 grams of iodide, and 0.202 gram of hydrogen were formed from the dissociation reaction, determine the partial pressure of the three components in the reaction: H2, I, and HI.
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At an altitude of 11,000 m (a typical cruising altitude for a jet airliner), the air temperature is -50.0 ∘C and the air density is 0.303 kg/m3. The molar mass of air is 28.8 g/mol. What is the pressure of the atmosphere at that altitude? (Note: The temperature at this altitude is not the same as at the surface of the earth, so the equation P=P0exp(−MgyRT)P=P0exp(−MgyRT) doesn't apply.) Express your answer with the appropriate units.

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