5. Consider a general reversible reaction: A+B- X+Yand answer the following questions.a. Describe what happens at equilibrium in terms of reaction rate and chemical concentrations?b. Write the expression for the equilibrium constant for the given reaction.6. Consider the following general reversible reaction is taking place in a reaction vessel andhas achieved a state of chemical equilibrium.A+2B 2XIf the following stresses are applied to this reaction at equilibrium, which direction (forward orbackward) will the equilibrium shift?a. Increase in concentration of AB. Decrease in concentration of XFactors Affecting Reaction Rate, Chemical Equilibrium and Le Chatelier'sPrincipleMAYtv

Since you have asked multiple question, we will solve the first question for you.If you want any…

and answer the following questions. a. Describe what happens at equilibrium in terms of reaction rate and chemical concentrati b. Write the expression for the equilibrium constant for the given reaction. 6. Consider the following general reversible reaction is taking place in a reaction vessel ar has achieved a state of chemical equilibrium. 2X A+2B.

and answer the following questions. a. Describe what happens at equilibrium in terms of reaction rate and chemical concentrati b. Write the expression for the equilibrium constant for the given reaction. 6. Consider the following general reversible reaction is taking place in a reaction vessel ar has achieved a state of chemical equilibrium. 2X A+2B.

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

61
12. A 2.50 L vessel contains 1.75 mole N₂, 1.75 mol H₂ and 0.346 mole NH3. What is the direction of reaction needed to attain equilibrium at 401 °C? The equilibrium constant Kc for the reaction is 0.50 at this temperature. N₂(g) + 3H₂(g) 2NH3(g)
Consider the following reaction equilibrium . PCI3(g) + Cl2(g) PCI5(g) For this reaction, Kc=2.5 x 10-4. Suppose you set up a mixture with each reactant at 4.5 M. In the space below, give the concentration of product at equilibrium. In your uploaded work, give the concentrations of each reactant at equilibrium.
For the reaction: COCI2 (g) + CO + Cl2 (g) (g) At 100°C the reaction has an equilibrium constant of 2.2 x 10-10, If 1.00 mole of phosgene (COCI2) is placed in a 10.0 L flask, calculate the concentration of carbon monoxide at equilibrium. Write your answer in standard form (not scientific notation).
Catalysts affect reaction rates, but do not change either the equilibrium or the spontaneity of a reaction. True or False.
2. Please don't write on a paper. I can't understand handwritten.
5. Calculate the concentration of the products of the following equilibrium when the equilibrium constant is 12.3 and the equilibrium concentration of NOBr₂ is 2.17 mol/L. NOBr₂ (g) NO(g) + Br₂(g) Answer: Submit your completed Assignment Booklet to Moodle at the end of this lesson.
1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-
which statement is true?
A reaction begins with a solution containing reactants but no products. When the reaction reaches equilibruim a) The enthalpies of the reactants and products are equal b) The concentrations of the reactants and products are equal c) The equilibrium constant has decreased relative to its value at the start of the reaction d) The forward and reverse rate constants are equal e) None of the above
14. The following reaction is allowed to come to equilibrium and then the volume is increased. Predict the effect of the indicated volume change once equilibrium is restored. H2O(g) + CO2(g) double arrow H2CO3(g) The reaction will shift right. The reaction will shift left. There will be no effect. Effect can not be determined from information provided.
For any reversible reaction containing a double arrow such as: Reactants ⟷⟷ Products the statement "equilibrium shifts to the right" means: Group of answer choices; - The reaction can only go in the forward direction. - The reaction can only go in the reverse direction. - A stress will cause a portion of reactants to disappear and some additional products to appear. - A stress will cause a portion of products to disappear and some additional reactants to appear