(a)
Interpretation:
Whether the position of equilibrium will shift to right or left when some amount of
Concept Introduction:
When product is removed the equilibrium is shifted to product side.
(b)
Interpretation:
Whether the position of equilibrium will shift to right or left when some amount of
Concept Introduction:
When reactant is added the equilibrium is shifted to product side.
(c)
Interpretation:
Whether the position of equilibrium will shift to right or left when some amount of
Concept Introduction:
When reactant is removed the equilibrium is shifted to reactant side.
(d)
Interpretation:
Whether the position of equilibrium will shift to right or left when temperature is increased for the following equilibrium.
Concept Introduction:
When temperature is increased for an endothermic reaction then the equilibrium is shifted to the product side.
(e)
Interpretation:
Whether the position of equilibrium will shift to right or left after a catalyst is added for the following equilibrium.
Concept Introduction:
When catalyst is added then activation energy is reduced and thus equilibrium is attained faster.
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Introduction to General, Organic and Biochemistry
- Use Le Chteliers principle to predict the direction of the equilibrium shift in the following equilibria when the indicated stress is applied: a. Ag+(aq)+Cl(aq)AgCl(s); some Ag+ is removed. b. 2HI(g)+heatH2(g)+I2(g); the system is heated. c. 6Cu(s)+N2(g)+heat2Cu3N(s); the system is cooled and some N2 is removed.arrow_forward7-32 A particular reaction has an equilibrium constant of 1.13 under one set of conditions and an equilibrium constant of 1.72 under a different set of conditions. Which conditions would be more advantageous in an industrial process that sought to obtain the maximum amount of products? Explain.arrow_forward7-40 Is there any change in conditions that change the equilibrium constant, K, of a given reaction?arrow_forward
- 7-71 You have a beaker that contains solid silver chloride (AgCl) and a saturated solution of Ag+ and CI- ions in equilibrium with the solid. You add several drops of a sodium chloride solution. What happens to the concentration of silver ions?arrow_forwardUse Le Chteliers principle to predict the direction of equilibrium shift in the following equilibria when the indicated stress is applied: a. 2A+B+heatC; some A is removed. b. 2A+B+heatC+D; the system is cooled. c. N2O42NO2; some NO2 is removed.arrow_forwardIf the concentrations of products and reactants are equal, is the system at equilibrium?arrow_forward
- 7-41 The equilibrium constant at 1127°C for the following endothermic reaction is 571: If the mixture is at equilibrium, what happens to K if we: (a) Add some H2S? (b) Add some H2? (c) Lower the temperature to 1000°C?arrow_forwardSuppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forward
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