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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 0.042 at a certain temperature. If 2.860 g of PCIS initially decomposes in a 700 mL closed container, what will the equilibrium concentration of PCIs be? PCI:(g) PCL(g) + CL(g) PREV NEXT Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or implify terms. [2.860 + x] = 0.042 [4.086 - 2x] O RESET [x] [2x] [2x] [2.860 + x] [2.860 - x] [2.860 - 2x] [0.01374 + x] [0.01374 - x) [0.01374 - 2x] [0.01982 + x] [0.01962 - 1] [0.01002 - 2x) [4.086 + x] [4.086 - x] [4.086 - 2x]

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 0.042 at a certain temperature. If 2.860 g of PCIS initially decomposes in a 700 mL closed container, what will the equilibrium concentration of PCIs be? PCI:(g) PCL(g) + CL(g) PREV NEXT Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or implify terms. [2.860 + x] = 0.042 [4.086 - 2x] O RESET [x] [2x] [2x] [2.860 + x] [2.860 - x] [2.860 - 2x] [0.01374 + x] [0.01374 - x) [0.01374 - 2x] [0.01982 + x] [0.01962 - 1] [0.01002 - 2x) [4.086 + x] [4.086 - x] [4.086 - 2x]

Chemistry
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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
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Question 42 of 44 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 0.042 at a certain temperature. If 2.860 g of PCIs initially decomposes in a 700 mL closed container, what will the equilibrium concentration of PCIs be? PCL(g) PCL(g) + CL(g) PREV 2 NEXT Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. [2.860 + x] Kc = = 0.042 [4.086 - 2x] O RESET [x] [2x] [2.860 + x] [2.860 - x] [2.860 - 21] [0.01374 + x] [0.01374 - x] [0.01374 - 2x] [0.01962 + x] 0.01962 - 1] [0.01062 - 2x] [4.086 + z] [4.086 - x] [4.086 - 2x]
Transcribed Image Text:Question 42 of 44 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 0.042 at a certain temperature. If 2.860 g of PCIs initially decomposes in a 700 mL closed container, what will the equilibrium concentration of PCIs be? PCL(g) PCL(g) + CL(g) PREV 2 NEXT Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. [2.860 + x] Kc = = 0.042 [4.086 - 2x] O RESET [x] [2x] [2.860 + x] [2.860 - x] [2.860 - 21] [0.01374 + x] [0.01374 - x] [0.01374 - 2x] [0.01962 + x] 0.01962 - 1] [0.01062 - 2x] [4.086 + z] [4.086 - x] [4.086 - 2x]
Question 42 of 44 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 0.042 at a certain temperature. If 2.860 g of PCs initially decomposes in a 700 ml closed container, what will the equilibrium concentration of PCIs be? PCL(g) PCls(g) + CL(g) 2 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. PCL(g) PCI:(g) CL(g) Initial (M) 0.01962 Change (M) 0.01962 - z Equilibrium (M) 2 RESET 2.860 0.01374 0.01962 4.086 0.01374 + x 0.01374 -x 0.01374 - 2x 0.01962 +: 0.01962 -x 2.860 + x 2.860 - x 2.860 - 2x 0.01962-2x 4.086 + z 4.086 - x 4.086-2x
Transcribed Image Text:Question 42 of 44 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 0.042 at a certain temperature. If 2.860 g of PCs initially decomposes in a 700 ml closed container, what will the equilibrium concentration of PCIs be? PCL(g) PCls(g) + CL(g) 2 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. PCL(g) PCI:(g) CL(g) Initial (M) 0.01962 Change (M) 0.01962 - z Equilibrium (M) 2 RESET 2.860 0.01374 0.01962 4.086 0.01374 + x 0.01374 -x 0.01374 - 2x 0.01962 +: 0.01962 -x 2.860 + x 2.860 - x 2.860 - 2x 0.01962-2x 4.086 + z 4.086 - x 4.086-2x
Expert Solution
Step 1

Kc denotes the ratio of concentration of the products to the reactants raise to the power of their stoichiometric coefficients when the reaction is in equilibrium.
Kc is a function of temperature depending upon the nature of reaction.

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