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A student placed O.236 mol of PCI3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction PCI3(3) + Cl2(g) 2 PCI5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCI3. What were the initial concentrations of the reactants and product? [PCI3] = i M [Cl2] = i M [PCI5) = i M

A student placed O.236 mol of PCI3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction PCI3(3) + Cl2(g) 2 PCI5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCI3. What were the initial concentrations of the reactants and product? [PCI3] = i M [Cl2] = i M [PCI5) = i M

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A student placed 0.236 mol of PCl3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction
PCl3(g) + Cl2(g) ⇄ PCl5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCl3.

A student placed O.236 mol of PCI3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction PCI3(3) + Cl2(g) 2 PCI5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCI3. What were the initial concentrations of the reactants and product? [PCI3] = i M [Cl2] = i M [PCI5) = i M By how much had the concentrations changed when the reaction reached equilibrium? The concentration of PCI3 has decreased by i M The concentration of Cl2 has decreased by i M The concentration of PCI5 has increased by i M What were the equilibrium concentrations? The equilibrium concentration of PCI3 = i M The equilibrium concentration of Cl2 = i M The equilibrium concentration of PCI5 = i M What is the value of K. for this reaction at this temperature? K =
Transcribed Image Text:A student placed O.236 mol of PCI3(g) and 0.145 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction PCI3(3) + Cl2(g) 2 PCI5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCI3. What were the initial concentrations of the reactants and product? [PCI3] = i M [Cl2] = i M [PCI5) = i M By how much had the concentrations changed when the reaction reached equilibrium? The concentration of PCI3 has decreased by i M The concentration of Cl2 has decreased by i M The concentration of PCI5 has increased by i M What were the equilibrium concentrations? The equilibrium concentration of PCI3 = i M The equilibrium concentration of Cl2 = i M The equilibrium concentration of PCI5 = i M What is the value of K. for this reaction at this temperature? K =
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