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 remove remove some add some remove some remove some some water solid carbon hydrogen carbon monoxide hydrogen add some carbon monoxide add some solid carbon 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 remove remove some add some remove some remove some some water solid carbon hydrogen carbon monoxide hydrogen add some carbon monoxide add some solid carbon 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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A scientist is studying how certain factors affect the rate of a particular reaction. She observes that under one set of conditions, the reaction proceeded much faster than under a different set of conditions. Identify the most likely sets of conditions that produced each reaction rate. Drag each item to the appropriate bin. • View Available Hint(s) Reset Help lower temperature larger quantities of reactants smaller quantities of reactants higher temperature Faster reaction Slower reaction
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.
A burner in a gas stove breaks propane and oxygen up to form carbon dioxide and water, thereby heating a home. Which part is the source of the activation energy required, and is this reaction endothermic or exothermic? The flame from the burner provides the energy to perform the reaction. The reaction is endothermic. The burning propane gas provides the energy to perform the reaction. The reaction is exothermic. The burning propane gas provides the energy to perform the reaction. The reaction is endothermic. The flame from the burner provides the energy to perform the reaction. The reaction is exothermic.
Consider the following general reaction for which gases A and B are mixed.in a constant volume container: A(g) + B(g) -> C(g) + D(g) According to collision theory, what happens to the rate of the reaction under the following changes: (consider each change separately) increase the temperature decrease the temperature increase the volume there is no change to the reaction rate A. decrease the volume the reaction rate increases В. decrease the pressure the reaction rate decreases C. collision theory does not allow you to predict the change in reaction rate increase the pressure D. decrease the concentration increase the concentration
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
QUESTION 15 Consider the following chemical reaction: Mg(s) + 2HCI(ag) MgCl2(aq) + H2(g) Which of the following changes will increase the rate of this reaction? O Decreasing the concentration of HCI. Decreasing the temperature. O Adding more MgCl2. O Adding a catalyst. O Increasing the pressure of H2. QUESTION 16 Click Save and Submit to save and submit. Click Save All Answers to save all answers. ch
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
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
For the exothermic reaction 4 NH3(g) +7 02(g)- => 4 NO2(g) + 6 H20(g) which change will increase the quantity of NO2 in the mixture? O A. increasing temperature OB. decreasing container volume OC. adding Ne(g) O D. adding H20(g) O E. adding a catalyst