Predict the equilibrium concentration of Ca²* in the reaction described below by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. Initial (M) Change (M) Equilibrium (M) CaCrO.(s) Ca²+ (aq) + CrO₂² (aq) 3 NEXT > A solid sample of CaCrO, dissolves in solution. Fill in the ICE table with the appropriate value for each involved species to determine the pressure of all reactants and products. = CaCrO.(s) 2 Ca²(aq) + CrO.² (aq)

Predict the equilibrium concentration of Ca²* in the reaction described below by constructing an ICE table, writing the equilibrium constant expression, and solving for the equilibrium concentration. Complete Parts 1-3 before submitting your answer. Initial (M) Change (M) Equilibrium (M) CaCrO.(s) Ca²+ (aq) + CrO₂² (aq) 3 NEXT > A solid sample of CaCrO, dissolves in solution. Fill in the ICE table with the appropriate value for each involved species to determine the pressure of all reactants and products. = CaCrO.(s) 2 Ca²(aq) + CrO.² (aq)

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 4ALQ: Given the reactionA(g)+B(g)C(g)+D(g), consider the following situations: i. You have 1.3 M A and 0.8...

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Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the interconversion reaction?
7-32 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.
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
The following data are for the system A(g)2B(g) (a) How long does it take the system to reach equilibrium? (b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 45 s? After 90 s?
For a typical equilibrium problem, the value of K and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
Summarize the steps for solving equilibrium problems (see the beginning of Section 12-6). In general, when solving an equilibrium problem, You should always set up an ICE table. What is an ICE table?
7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.
Le Chteliers principle is stated (Section 12-7) as follows: If a change is imposed on a system at equilibrium, the position of the equilibrium will shift in a direction that tends to reduce that change. The systemN2(g)+3H2(g)2NH3(g) is used as an example in which the addition of nitrogen gas at equilibrium results in a decrease in H2 concentration and an increase in NH3, concentration. In the experiment the volume is assumed to be constant. On the other hand, if N2 is added to the reaction system in a container with a piston so that the pressure can be held constant, the amount o f NH3 actually could decrease, and the concentration of H2 would increase as equilibrium is reestablished. Explain how this can happen. Also, if you consider this same system at equilibrium, the addition of an inert gas. holding the pressure constant, does affect the equilibrium position. Explain why the addition of an inert gas to this system in a rigid container does not affect the equilibrium position.
The equilibrium between nitrogen monoxide, oxygen, and nitrogen dioxide may be expressed in the equation 2NO(g)+O2(g)2NO(g). Write the equilibrium constant expression for this equation. Then express the same equilibrium in at least two other ways, and write the equilibrium constant expression for each. Are the constants numerically equal? Cite some evidence to support your answer. Nitrogen monoxide and oxygen, both colorless gases, react to form reddish-brown nitrogen dioxide.
Given the reactionA(g)+B(g)C(g)+D(g), consider the following situations: i. You have 1.3 M A and 0.8 M B initially. ii. You have 1.3 M A, 0.8 M B. and 0.2 M C initially. iii. You have 2.0 M A and 0.8 M B initially. Order the preceding situations in terms. of increasing equilibrium concentration of D. Explain your order. Then give the order in terms of increasing equilibrium concentration of B and explain.
. In general terms. what does the equilibrium constant for a reaction represent? What is the algebraic form of the equilibrium constant for a typical reaction? What do square brackets indicate when we write an equilibrium constant?