Sciencecourse.apexlearning.com/pPretest: Unit 8Question 4 of 25Ammonia (NH3) can be made using the reversible reaction shown. Whichchange would keep this reaction from shifting to form more of the product?3H2 + N2 = 2NH3 + energy+A. Removing NH3 from the reaction vessel as it formsB. Decreasing the temperature in the reaction vesselC. Removing N₂ from the reaction vessel as it formsD. Decreasing the pressure in the reaction vesselSUBMIT2ZA:Apex Learni

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Ammonia (NH3) can be made using the reversible reaction shown. Which change would keep this reaction from shifting to form more of the product? 3H2 + N2 2NH3 + energy OA. Removing NH3 from the reaction vessel as it forms OB. Decreasing the temperature in the reaction vessel OC. Removing N₂ from the reaction vessel as it forms OD. Decreasing the pressure in the reaction vessel SUBMIT

Ammonia (NH3) can be made using the reversible reaction shown. Which change would keep this reaction from shifting to form more of the product? 3H2 + N2 2NH3 + energy OA. Removing NH3 from the reaction vessel as it forms OB. Decreasing the temperature in the reaction vessel OC. Removing N₂ from the reaction vessel as it forms OD. Decreasing the pressure in the reaction vessel SUBMIT

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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Suppose the reaction system: UO2 (s) + 4 HF (g) ← UF4 (g) + 2 H₂O (g) has already reached equilibrium. Predict the effect that each of the following changes will have on the direction of the reaction to reestablish equilibrium. Indicate whether the reaction will shift to the left, to the right, or no change. a. Additional UO2 is added to the system. b. The reaction is performed in a glass reaction container and the HF begins to react with the glass. c. Water vapor is removed. d. The pressure is increased.
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Can you help me every step by step with number 3 part A, part B, part C, part D? Can you explain it to me?
Suppose you have the following chemical reaction at equilibrium: N2H4 (1) + N2O4 (1) = N2 (g) + H2O (g) If this reaction releases heat, what direction will the equilibrium shift when: 1. the amount of N2 is decreased? 2. the heat of the system is increased? 3. an inert gas with pressure 3.00 atm is placed in the system? 4. the volume of the system is reduced? 5. a catalyst in the reaction is placed?
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adding some CO(g) increasing the volume of the container removing some H₂O(g) Shifts in the direction of the products Shifts in the direction of the reactants chill the reaction removing H₂(g) as it forms Equilibrium does not change
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Which of the following is correct? A. When Qc > Kc, The ratio of initial concentrations of products to reactants is too large. To reach equilibrium, reactants must be converted to products B. When Qc > Kc, The ratio of initial concentrations of products to reactants is too large. The system proceeds from right to left to reach equilibrium. C. When Qc < Kc, The ratio of initial concentrations of products to reactants is too small. To reach equilibrium, products must be converted to reactants D. When Qc < Kc, The ratio of initial concentrations of products to reactants is too small. The systems proceeds right to left to reach equilibrium.
23. What happens when a chemical reaction reaches equilibrium? The amounts of reactants and products remain constant because the reaction stops. The reaction stops because the concentration of reactants is too low to sustain it. The reaction reverses so some of the products are converted back into reactants. The rate of the forward reaction is the same as the rate of the reverse reaction. PREVIOUS 23 of 25 NEXT REVIEW