CHEM 102 Optional Assignment: A sample of PCIs was placed in a vessel with an original concentration of 0.40 M. After the PCI, has decomposed and equilibrium has been established, 25% of the PCls remains. PCI5(g) PC13(g) + Cl₂(g) What are the equilibrium concentrations of PCI5, PCI3, and Cl₂? Write the equilibrium constant expression of the decomposition reaction Calculate the equilibrium constant for decomposition reaction

CHEM 102 Optional Assignment: A sample of PCIs was placed in a vessel with an original concentration of 0.40 M. After the PCI, has decomposed and equilibrium has been established, 25% of the PCls remains. PCI5(g) PC13(g) + Cl₂(g) What are the equilibrium concentrations of PCI5, PCI3, and Cl₂? Write the equilibrium constant expression of the decomposition reaction Calculate the equilibrium constant for decomposition reaction

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 118CP: Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain...

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The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
A 4.72-g sample of methanol (CH3OH) was placed in an otherwise empty 1.00-L flask and heated to 250.C to vaporize the methanol. Over time, the methanol vapor decomposed by the following reaction: CH3OH(g)CO(g)+2H2(g) After the system has reached equilibrium, a tiny hole is drilled in the side of the flask allowing gaseous compounds to effuse out of the flask. Measurements of the effusing gas show that it contains 33.0 times as much H2(g) as CH3OH(g). Calculate K for this reaction at 250.C.
Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
7-22 If you add a piece of marble, CaCO3 to a 6 M HCI solution at room temperature, you will see some bubbles form around the marble as gas slowly rises. If you crush another piece of marble and add it to the same solution at the same temperature, you will see vigorous gas formation, so much so that the solution appears to be boiling. Explain.
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Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
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