By how much had the concentrations changed when the reaction reached equilibrium?The concentration of PCI3 has decreased by iMThe concentration of Cl, has decreased by iThe concentration of PCI5 has increased byiWhat were the equilibrium concentrations?The equilibrium concentration of PCI3 =!The equilibrium concentration of Cl2 =!MThe equilibrium concentration of PCI5 =i!MWhat is the value of K. for this reaction at this temperature?K =i-- A student placed 0.264 mol of PCI3(g) and O.180 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reactionPCI3(g) + Cl2(g)2 PCI5(g) came to equilibrium it was found that the flask contained 0.120 mol of PCI3.

A student placed 0.264 mol of PCI3 (g) and 0.180 mol of Cl₂(g) into a 1.00 liter container at 250…

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 %3D What is the value of K. for this reaction at this temperature? Kc = i

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 %3D What is the value of K. for this reaction at this temperature? Kc = i

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

Section: Chapter Questions

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 0.227 mol of PCI3(g) and 0.134 mol of Cl2(g) into a 1.00 liter container at 250 °C. After the reaction PCI3(g) + 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 [Cl2] = i M [PCI5] = i By how much had the concentrations changed when the reaction reached equilibrium? The concentration of PCI3 has decreased by i The concentration of Cl, has decreased by i The concentration of PCI5 has increased by i M
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