At a certain temperature, the equilibrium constant K for the following reaction is 0.0071: Cl₂(g) + CHCl3(g) → HC1(g) + CC14(g) 2 Use this information to complete the following table. There will be very little Cl₂ and CHCI 3. Suppose a 20. L reaction vessel is filled with 1.8 mol of Cl₂ and 1.8 mol of CHCl3. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little HCI and CCI4. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 HCl(9)+CC14(9) Cl₂(9)+CHC13 (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 2 Cl₂(9)+2CHC13 (9) 2 HCl(9)+2CC14(9)

At a certain temperature, the equilibrium constant K for the following reaction is 0.0071: Cl₂(g) + CHCl3(g) → HC1(g) + CC14(g) 2 Use this information to complete the following table. There will be very little Cl₂ and CHCI 3. Suppose a 20. L reaction vessel is filled with 1.8 mol of Cl₂ and 1.8 mol of CHCl3. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little HCI and CCI4. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 HCl(9)+CC14(9) Cl₂(9)+CHC13 (9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 2 Cl₂(9)+2CHC13 (9) 2 HCl(9)+2CC14(9)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 60QRT

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Similar questions

During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium constant, Kc, is 0.60 for PCl5(g) PCl3(g) + Cl2(g) Calculate the concentrations of all species after equilibrium has been reached.
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species. (b) The volume of the container is decreased to 4.5 L and the system allowed to return to equilibrium. Calculate the new equilibrium concentrations. (Hint: The calculation will be easier if you view this as a new problem with 0.5 mol of COBr2 transferred to a 4.5-L flask.) (c) What is the effect of decreasing the container volume from 9.50 L to 4.50 L?
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?

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