For each of the following changes to the equilibrium system below, predict which reaction will be favored - forward (to the right), reverse (to the left), or neither. H2(gas) + Cl2(gas) = 2HClgas) + Heat Adding chlorine gas will cause the equilibrium to shift to [Select] • Removing hydrogen chloride gas will.cause the equilibrium to shift to [ Select] • Increasing the pressure on the system will cause the equilibrium to shift to [Select ] Decreasing the pressure on the system will cause the equilibrium to shift to [Select] • Removing hydrogen gas will cause the equilibrium to shift to [ Select ]

For each of the following changes to the equilibrium system below, predict which reaction will be favored - forward (to the right), reverse (to the left), or neither. H2(gas) + Cl2(gas) = 2HClgas) + Heat Adding chlorine gas will cause the equilibrium to shift to [Select] • Removing hydrogen chloride gas will.cause the equilibrium to shift to [ Select] • Increasing the pressure on the system will cause the equilibrium to shift to [Select ] Decreasing the pressure on the system will cause the equilibrium to shift to [Select] • Removing hydrogen gas will cause the equilibrium to shift to [ Select ]

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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In an ammonia reaction if the temperature is increased which direction will equilibrium shift? If the reaction is exothermic is it better to heat or cool the product to yield more ammonia? In what ways are temperature and equilibrium related?
Consider the following reaction at equilibrium taking place in the gas phase: N2O + 2 H2O double arrows NH4NO3 In what direction will the equilibrium shift if the volume of the container is increased? Towards reactants Towards products Neither
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Question 26 4 pts Given the following equilibrium reaction, identify the effect each change will have as the reaction shifts to reestablish equilibrium. 2NO2 (g) N2O4 (g) AH = -55 kJ Decide if each change would cause the reaction to shift to favor reactants, products, or cause no change. Change Effect on Equilibrium Decrease in the temperature [Select] Decrease the volume [Select] Decrease in reactants [Select] Add a catalyst [Select] > > >
A change in temperature changes the composition at equilibrium because O equilibrium constants depend on temperature. more molecules have enough kinetic energy. O the reverse reaction is not dependent on temperature. the rate of the forward reaction is increased.
when 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…
19. How will increasing the pressure in the reaction vessel affect the equilibrium of this reaction? 4NH, (g)+50,(g) =4NO(g)+6H,0(g) O shift equilibrium to the left because there are fewer gas molecules on the left O shift equilibrium to the left because oxygen is never part of the equilibrium constant shift equilibrium to the right because water is not affected by a pressure chinge O shift equilibrium to the right because the molecules are smaller on the right PREVIOUS AMC Lit op
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}
For 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"]
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12. Use Le Châtelier's principle to predict what will happen if the temperature of the following equilibrium system is decreased. The reaction in the forward direction is endothermic. 4C1 Co(H₂O) pink 1 CoCl₂ + 6H₂O purple/blue A) The equilibrium will shift to the left. B) The equilibrium solution will become more purple. C) The equilibrium will shift to the right. D) The concentration of chloride ion will decrease. E) There will be no change.
7. Given the following equilibrium systems, note the direction the equilibrium will shift [→,-, NC, no change] when the named "stress" is applied. 2 NH3(g) + 92.5 kJ a 1 2 3 4 5 6 7 Stress Remove N2 (g) Add NH3 (9) Remove H2 (9) Remove NH3 (g) Add O2 (g) Decrease Pressure Add Heat N2(g) + 3 H2 (g) Equilibrium Shift