Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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In general, for a system at equilibrium, indicate the direction the equilibrium will shift for the following change. The concentration of one or more of the products is decreased.
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- Why can an equilibrium be represented mathematically? Discuss the role collisions play in equilibrium reactions.arrow_forwardwhen an equilibrium is disrupted (“stressed”) due to changes that a chemist imposes on the system, Le Chatelier’s Principle predicts that the equilibrium will shift in the direction that will undo as much of the change as possible. For instance, if a particular reactant compound is removed through some chemical means, then the equilibrium will shift to favor the reactants, so as to replace some of the lost compound. In this lab, you will observe the effects of stress on the tetrachlorocobaltate(II)/hexaquocobalt(II) equilibrium shown below: CoCl42-(solv) + 6 H2O(solv) Co(OH2)62+(solv) + 4 Cl-(solv) blue pink The (solv) means a solvated species. In this system, ethanol is the solvent. This means that water can not be excluded from the reaction quotient any longer, since it is now a solute in ethanol and therefore has a measurable concentration. The color of the solution provides a visual clue about the dominant cobalt species…arrow_forward29.arrow_forward
- The following reactions start at equilibrium.A stress is added and the position of equilibrium shifts. After the indicated stress is added which of the following reactions will proceed towards products?The added stress is the part listed inside the braces {} HINT: You must be careful now because this is a trick question. To answer this question, I suggest that you first write the equilibrium expression. Then recall what must be true for the concentration of pure solids and liquids in an equilibrium expression. See section Heterogeneous Equilibria, p.130 in the notes. AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) {and some but not all AgCl(s) is removed} Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g) {and CO2(g) is removed} Ni(s) + Cl2(g) NiCl2 {and more Ni(s) is added}arrow_forwardFor the generalized chemical reaction A(g) + B(g) C(g) + D(g) determine whether the concentration of D in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a) concentration of C is increased [ Select ] ["increase", "decrease", "no change"] b) concentration of C is decreased [ Select ] ["increase", "decrease", "no change"]arrow_forwardExplain Le Chatelier's principle as it relates to chemical equilibrium. Describe the types of stresses that cause chemical reactions and equilibrium to make more products. Use details to support your answerarrow_forward
- Consider 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_forwardDecide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction. d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) 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_forwardIn general, for a system at equilibrium, indicate the direction the equilibrium will shift for the following change. The concentration of one or more of the products is increased.arrow_forward
- The addition of a catalyst will change the composition of the equilibrium mixture. True Falsearrow_forwardRecord your two digit answer. Use the following information to answer the next 4 questions. An equilibrium system was established in a 1.00 L flask at a certain temperature as represented by the following equation ICI(g) + Cl₂(g) ICI,(g) + energy brown yellow-green bright yellow At equilibrium the flask contained 0.0571 mol of ICI(g), 1.07 mol of Cl₂(g), 1.87 mol of ICl3(g) The value of the equilibrium constant for this system is 30.6 Record your 3-digit answer Under these conditions, the equilibrium system in Question 20 favours the forward the reverse neither reaction. ?arrow_forwardPicturearrow_forward
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