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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1. Consider the following reaction at 500 K: 2 NO (g) + O2 (g) 2 2 NO2 (g); Kc = 6.9 x 105 This reaction is allowed to reach equilibrium, and then analyzed and found to contain the following concentrations: [O2] = 1.0 x 10-3 M [NO2] = 5.0 x 10-2 M. Determine the equilibrium concentration of NO (g).
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Consider the reaction A + B C+D, which has an equilibrium constant, K, equal to 3.4 x 102. If one begins a reaction by placing 0.600 moles of A in a 1.0 L container as well as 0.150 moles of 1. B, what will be the equilibrium concentrations of A, B, C, and D? Write your answers in the spaces provided below. a. [А] b. [B]= [C]= С. d. [D]= Once the reaction in problem 1 reaches equilibrium, some additional B is injected into the flask 2. from an outside source. LeChatelier's principle says the reaction will (circle one): be unchanged shift to the right shift to the left Pyridine is a weak base with a Kb 1.7 x 109. If 0.300 moles of pyridine is added to 1.00 L of 3. water, what will be the equilibrium concentrations of the species below: a. [Pyridine] = b. [Pyridine-H] (the pyridinium ion) [ОН-] 3 С. What is the pH of the solution in problem 4 (above)? .