For the reactionC(s) + H2O(g) = H2(g) + CO(g)classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the reaction. Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help add some salid carbon remove some water add some remove somn remove some hrydrogen carban monoxide solid carbon add some carbon monoxide remave some hydragen add some water Leftward shift Rightward shift No shift

For the reactionC(s) + H2O(g) = H2(g) + CO(g)classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the reaction. Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help add some salid carbon remove some water add some remove somn remove some hrydrogen carban monoxide solid carbon add some carbon monoxide remave some hydragen add some water Leftward shift Rightward shift No shift

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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⦁ 4. Make your own energy diagram for an exothermic reaction that does not include a catalyst and one with a catalyst (Be sure each line is a different color or labeled). Label the axis of the diagram. Then, state what a catalyst is and how a catalyst affects the reaction rate.
Catalysts increase reaction rates by _____ A) increasing the activation energy. B) increasing the enthalpy of reaction. C) decreasing the enthalpy of reaction. D) providing an alternate reaction mechanism with a lower activation energy. E) changing the value of the equilibrium constant.
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.
(Write a three-paragraph summary that answers the guiding question: Do Changes in Temperature, Reactant Concentration, and Product Concentration Affect the Equilibrium Point ofa Reaction?) Discussion: F5 F6 F7 F8 PrtSc Insert F9 F10 F11 F12 & * 8 T. Y 5
Part A Consider the following reaction in chemical equilibrium: COC1₂ (g) CO(g) +Cl₂ (g) What is the effect of adding additional CO(g) to the reaction mixture? What is the effect of adding additional COC12 (g)? Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. Submit right Cl₂ CO left COC12 Request Answer < Return to Assignment Adding COC2 increases the concentration of progress to shift to the Adding CO increases the concentration of to shift to the (away from the Provide Feedback " " |). Reset causing the reaction Help causing the reaction progress
Assume that the reaction below is at equilibrium. A stress is then applied as described. Click on the appropriate circle to indicate how the system will respond to the stress. 2H2(g) + O2(g) →2H20(g) H=-10KJ H2 is removed. and the cow jumped over the moon shift to the right shift to the left no change
5. Study the following reactions: 2H2O2⇌2H2O+O22H2O2⇌catalyst2H2O+O2Reaction 1: uncatalyzedReaction 2: catalyzed If the two reactions occur at the same temperature, which statements are true? Select all that apply. The catalyzed reaction will reach equilibrium faster than the uncatalyzed reaction. The uncatalyzed reaction will reach equilibrium faster than the catalyzed reaction. The equilibrium position of the catalyzed reaction is greater than that of Reaction 1. The equilibrium position is the same in both the catalyzed reaction and the uncatalyzed reaction. The equilibrium position of the catalyzed reaction is shifted toward the products side. The equilibrium position of the catalyzed reaction is shifted toward the reactants side.
Which of the following will lower the activation energy for a reaction? Group of answer choices raising the temperature of the reaction. increasing the concentrations of reactants. increasing the surface area of the reactants. adding a suitable catalyst.
Question 17 A chemistry student wants to speed up her reaction. Which of the following would be the best ways for her to do this? Select all that apply. Select 3 correct answer(s) | Increase the amount of product | Increase the amount of reactant Add a catalyst Decrease the temperature Increase the temperature
d. Suppose you add compound E to the equilibrium mixture. Compound E reacts with compound D which is a component of the equilibrium to form compound F as described in the equation below. E + D Which compound is removed from the equilibrium mixture when you add compound E to the mixture? (Enter "correct" for ALL correct answers.) • B D e. What shift in the equilibrium will occur as a result of the addition of compound E? (Enter "correct" for the correct shift.) A + B C + D (shift to the right) A + B C + D (shift to the left)
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
Problem-Solving Strategies: Understanding Equilibrium ▼ Part A Identify the stress Consider the equilibrium reaction CO(g) + H₂O(g) - CO₂(g) + H₂(g) Determine how each change in the left-hand column will stress the system and in which direction the equilibrium reaction will shift in response. Drag the appropriate labels to their respective targets. ► View Available Hint(s) Increase reactant Decrease reactant Increase product Decrease product Submit Type here to search Reverse reaction rate temporarily increases Forward reaction rate temporarily increases Forward reaction rate temporarily decreases Reverse reaction rate temporarily decreases Change Add CO(g) Remove H₂O(g) Add CO₂(g) Remove H₂(g) I H System stress Group 1 Group 1 Group 1 Group 1 ✔ Ca Equilibrium shift Group 2 Group 2 Group 2 Group 2 Reset Help