PC13(g)+Cl2(g)ZPCI5(g)Kc=0.11 A 0.60mol sample of PC13 and a 0.70mol sample of Cl2(g) are placed in a previously evacuated 1.0L rigid container, and the reaction represented above takes place. At equilibrium, the concentration of PCI5(g) in the container is 0.040M 0.70 0.60 0.50 0.40 0.30 0.20 0.10 0.00 Time 1) On the graph above, draw three curves, one for each of the three gases. The curves must show how the concentration of each of the three gases changes as equilibrium is established. Label each curve with the formula of the gas. 2) Explain how the slopes of the curves at equilibrium can be used to show that the rates of the forward and reverse reactions are the same at equilibrium. 3) As the reaction occurs at constant temperature, does the pressure inside the container increase, decrease, or remain the same? Explain why Concentration (M)

PC13(g)+Cl2(g)ZPCI5(g)Kc=0.11 A 0.60mol sample of PC13 and a 0.70mol sample of Cl2(g) are placed in a previously evacuated 1.0L rigid container, and the reaction represented above takes place. At equilibrium, the concentration of PCI5(g) in the container is 0.040M 0.70 0.60 0.50 0.40 0.30 0.20 0.10 0.00 Time 1) On the graph above, draw three curves, one for each of the three gases. The curves must show how the concentration of each of the three gases changes as equilibrium is established. Label each curve with the formula of the gas. 2) Explain how the slopes of the curves at equilibrium can be used to show that the rates of the forward and reverse reactions are the same at equilibrium. 3) As the reaction occurs at constant temperature, does the pressure inside the container increase, decrease, or remain the same? Explain why Concentration (M)

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...

See similar textbooks

Similar questions

H2 + I2 → 2 HI At a certain temperature, the Kc of this reaction is 58.2. At this temperature, 5.00 mol H2 and 5.00 mol I2 were placed in a 0.500 L container to react. What concentration of HI is present at equilibrium?
Phosphorus pentachloride decomposes at high temperatures. PCl5 = PCl3 + Cl2 An equilibrium mixture at some temperature consists of 3.56 g of PCl5 , 4.86 g of PCl3 , and 3.59 g of Cl2 in a 1.00-L flask. What will the concentration of PCl5 be when equilibrium is reestablished after addition of 1.31 g Cl2?
The equilibrium constant for the following reaction is 0.18 at a set temperature. Find the equilibrium concentrations if the initial concentration of PCl3 is 0.225 mol/L and the initial concentration of Cl2 is 0.150 mol/L. PCI3(g)+CI2(g)=PCI5(g)
The equilibrium constant, K, for the following reaction is 1.37×10-2 at 503 K. PCl5 (g) PCl3 (g) + Cl2 (g) An equilibrium mixture of the three gases in a 13.9 L container at 503 K contains 0.303 M PCl5, 6.44×10-2 M PCl3 and 6.44×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 6.07 L? [PCl5] = M [PCl3] = M [Cl2] = M
Consider the reaction. PCI, (g) = PCI, (g) + Cl,(g) K. = 0.0420 The concentrations of the products at equilibrium are [PC13] = 0.140 M and [Cl2] = 0.170 M. What is the concentration of the reactant, PCI5 , at equilibrium? [PC!5] = M
22) The ke for the equilibrium shown below is 45. Some methane and hydrogen sulfide are added to a container and at equilibrium the concentrations of methane and hydrogen sulfide are found to be 0.22 mol/L and 0.33 mol/L respectively. What are the equilibrium concentrations of carbon disulfide and hydrogen gas? CH4 + 2H2S(g) → CS2 (g) 4H2
None
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 510 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 7.99 L container at 510 K contains 0.377 M PCl5, 8.23×10-2 M PCl3 and 8.23×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 18.5 L? [PCl5] = M [PCl3] = M [Cl2] = M
Consider the equilibrium between SbCl5, SbCl3 and Cl₂. SbCl5(g) SbCl3(g) + Cl₂(g) K = 2.46x10-² at 530 K The reaction is allowed to reach equilibrium in a 7.30-L flask. At equilibrium, [SbCl5] = 0.430 M, [SbCl3] = 0.103 M and [Cl₂] = 0.103 M. (a) The equilibrium mixture is transferred to a 14.6-L flask. In which direction will the reaction proceed to reach equilibrium? (b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 14.6-L flask. [SbCl5] = [SbCl3] = [Cl₂] |||| ΣΣΣ