Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Consider the gas-phase reaction of ethylene (CH 2 CH 2) with hydrogen to form ethane (C 2H 6), which occurs in the presence of a palladium catalyst (Section 6.4B). a. Write the expression for the equilibrium constant for this reaction. b. If ΔH = −28 kcal/mol, are the products or reactants higher in energy? c. Which is likely to be true about the equilibrium constant for the reaction: K > 1 or K < 1? d. How much energy is released when 20.0 g of ethylene reacts? e. What happens to the rate of the reaction if the concentration of ethylene is increased? f. What happens to the equilibrium when each of the following changes occurs: [1] an increase in [H 2]; [2] a decrease in [C 2H 6]; [3] an increase in temperature; [4] an increase in pressure; [5] removal of the palladium catalyst?arrow_forwardUse Le Chatelier’s principle to determine whether the equilibrium for the exothermic reaction below shifts to the left, right, or does not change under each condition listed: N2(g) + 3H2(g) → 2NH3(l) Some hydrogen is added A catalyst is added The temperature is raised The pressure is decreased by increasing the volume of the containerarrow_forwardCan you show me how to answer this type of question I found on a online practice organic chemistry review.arrow_forward
- The reaction quotient (Q) for a system is 70. If Kc = 35, what will happen as equilibrium is approached? Othere will be a net gain in product the reaction is at equilibrium O there will be no net gain in either product or reactant. there will be a net gain in reactant there will be a net gain in both reactant and productarrow_forwardWhich of the following explains the term "dynamic" as applied to chemical equilibrium? Group of answer choices The reaction continues to convert reactants to products, and products to reactants when the concentrations are equal , but with no net change in concentration at equilibrium. Products can form reactants until equilibrium is established. Reactants can form products until equilibrium is established. The reaction continues to convert reactants to products, and products to reactants when the reaction rates are equal, but with no net change in concentration at equilibrium. The reaction stops when equilibrium is reached.arrow_forwardSuppose the reaction system: UO₂ (s) + 4HF (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 HF 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 added. d. The volume is increased.arrow_forward
- Label the following statements as true or false.True False When Q < Kc, the reaction shifts to the left to reduce stress on the system. True False When a system is at equilibrium, the reactants and the products of the reaction will be equal in concentration. True False When a system is at equilibrium, the reaction rate of the forward reaction is less than to the reaction rate of the reverse reaction. True False When Q > Kc, the reaction shifts to the right to reduce stress on the system. True False For a reversible reaction, the ΔH of the forward reaction is equal in magnitude but opposite in sign to the ΔH of the reverse reaction. True False If Kc=5 for the reaction A + B <--> AB, then AB <--> A + B has a Kc=0.2arrow_forwardAnalyze both reactions and indicate whether the equilibrium tends to favor the reactants or the products. Reaction A: H30* + NH,* NH2 HO, Reaction B: + "OH + ОН Select the true statement(s). Reactions A and B tend to favor the products. Reactions A and B tend to favor the reactants. Reaction A tends to favor the reactants, Reaction B favors the products. Reaction A tends to favor the products, Reaction B favors the reactants.arrow_forwardFor the reaction: 2HBr → H2 + Br2 ΔH = -17.4 kcal/mol. And Keq = 32 X 10 20 Is the reaction exothermic or endothermic? Are products or reactants favored? Using Le Chatelier’s Principle, what happens to the equilibrium if the concentration of Br2 is increased? Using Le Chatelier’s Principle, what happens to the equilibrium if the concentration of H2 is decreased?arrow_forward
- 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?arrow_forward4. Write an equilibrium equation, keq for the following reactions: a. N2 (g) + 3H2 (g) → 2NH3 (g) b. H2 (g) + I2 (g) → 2HI (g)arrow_forwardDecide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). B) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.arrow_forward
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