A student placed 0.354 mol of PCI3(g) and 0.293 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] = [Cl,] = [PCI5] = By how much had the concentrations changed when the reaction reached equilibrium? The concentration of PCI3 has decreased by i M The concentration of Cl, has decreased by M The concentration of PCI- has increased by What were the equilibrium concentrations? The equilibrium concentration of PCI3 = The equilibrium concentration of Cl2 = M The equilibrium concentration of PCI5 = M What is the value of Ke for this reaction at this temperature? K =

A student placed 0.354 mol of PCI3(g) and 0.293 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] = [Cl,] = [PCI5] = By how much had the concentrations changed when the reaction reached equilibrium? The concentration of PCI3 has decreased by i M The concentration of Cl, has decreased by M The concentration of PCI- has increased by What were the equilibrium concentrations? The equilibrium concentration of PCI3 = The equilibrium concentration of Cl2 = M The equilibrium concentration of PCI5 = M What is the value of Ke for this reaction at this temperature? K =

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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