Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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What kind of reaction alters the equilibrium? What is the effect of the addition of HCl to the equilibrium?
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- Methane and hydrogen sulfide react to form hydrogen and carbon disulfide, like this: CH₂(g)+2H₂S(g) → 4H₂(g)+CS₂(g) Use this chemical equation to answer the questions in the table below. Suppose 165. mmol of CH4 and 330. mmol of H₂S are added to an empty flask. How much H₂ will be in the flask at equilibrium? Suppose 165. mmol of H, and 41.3 mmol of CS, are added to an empty flask. How much H₂ will be in the flask at equilibrium? None. O Some, but less than 660. mmol. O 660. mmol. O More than 660. mmol. O None. O Some, but less than 165. mmol. O165. mmol. More than 165. mmol. X Sarrow_forwardWhen a reaction is said to have reached equilibrium, it means A- The reaction in both directions have stopped. B- The rate of the forward reaction is higher than that of the reverse reaction. C- The concentration of reactant and product are equal. D- The concentration of reactant and products do not change over time. E- The rate of the forward reaction is lower than that of the reverse reaction.arrow_forwardPart III Short Answer 10. List 3 important factors for a reaction to reach equilibrium. Explain why these factors are necessary to reach equilibrium. 1) 2) 3)arrow_forward
- What is meant by a reaction being at equilibrium? * useing Le Chateliers Principlearrow_forwardConsider the reversible reaction. PCl5↽−−⇀PCl3+Cl2 What substances are present at equilibrium? Cl2Cl2 PCl3PCl3 PCl5PCl5 Are the concentrations of phosphorus pentachloride, PCl5,PCl5, and phosphosphorus trichloride, PCl3,PCl3, constant or changing at equilibrium? The concentrations of both PCl5PCl5 and PCl3PCl3 are changing at equilibrium. The concentrations of both PCl5PCl5 and PCl3PCl3 are constant at equilibrium. The concentration of PCl5PCl5 is constant, and the concentration of PCl3PCl3 is changing at equilibrium. The concentration of PCl5PCl5 is changing, and the concentration of PCl3PCl3 is constant at equilibrium. How does the equilibrium change if more chlorine, Cl2,Cl2, is added to the reaction? The equilibrium shifts to the left. The equilibrium shifts to the right. The equilibrium does not shift to either the left or the right. If more phosphorus pentachloride, PCl5,PCl5, is added, how does the equilibrium change? The equilibrium…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
- What are the Step to be followed to determining acidity using hybridization effects ?arrow_forwardWhich is the appropriate description to show the effect of a catalyst on the reaction rate and equilibrium in a reversible reaction: Reactants › Products O• The rate of the forward reaction is increased. • The rate of the reverse reaction is decreased 0 •The equilibrium position is displaced to the right O • The rate of the forward reaction is increased. The rate of the reverse reaction is increased The equilibrium position is unchanged. • The rate of the forward reaction is increased. 0 •The rate of the reverse reaction is unchanged • The equilibrium position is displaced to the right • The rate of the forward reaction is unchanged. The rate of the reverse reaction is unchanged The equilibrium position is unchanged. Suppose that an exothermic reaction, Reactants < › Products, is at equilibrium. According to Le Chatelier's Principle, if the reaction temperature is increased, in which direction will the equilibrium be displaced? O The equilibrium will be displaced toward the…arrow_forwardConsider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed? a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increasesarrow_forward
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