These are three parts and it counts as one question. At 25 °C, K. =1 x 10-85 for the reaction%3D7102 (aq) + 9H20 + 7H (aq) = I2(aq) + 5H5IO6(aq)What is the value of K. for the following reaction?I2(aq)+ 5H5I0 710, (aq) + 9H,0 + 7H*(aq)Enter your response in scientific notation, e.g. enter 2E3 for 2000Kc = At 25 °C, K. = 1 x 10-85 for the reaction7103 (aq) + 9H20 + 7H*(aq) = 1(aq) + 5H,I0g(aq)What is the K, expression for the reaction?Use the following abbreviations in the Ke expression:K for Ke(I03) for [IO3](H2O) for [H20]H for [H+](12) for [I2](H5I06) for [H5IOg]EditWhat is the value of K, expression for the following reaction?I2(aq) + 5H5IO6(ag) 7103 (aq) + 9H20 + 7H (aq)Use the following abbreviations in the Ke expression:K for K.(103) for [IO2)(H2O) for [H20]H for [H*](12) for [I2](H5IO6) for [HSIOG]

1) Write the expression for Kc for the first reaction. 2) Write the expression for Kc the reverse…

At 25 °C, Kc =1 x 10-85 for the reaction %3D 7103 (aq) + 9H20 + 7H+(aq) e I2(aq) + 5H5IO5(aq) What is the value of K. for the following reaction? I2(aq) + 5H5IOg(aq) = 7103 (aq) + 9H,0 + 7H*(aq) Enter your response in scientific notation, e.g. enter 2E3 for 2000

At 25 °C, Kc =1 x 10-85 for the reaction %3D 7103 (aq) + 9H20 + 7H+(aq) e I2(aq) + 5H5IO5(aq) What is the value of K. for the following reaction? I2(aq) + 5H5IOg(aq) = 7103 (aq) + 9H,0 + 7H*(aq) Enter your response in scientific notation, e.g. enter 2E3 for 2000

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 2RQ: What is the law of mass action? Is it true that the value of K depends on the amounts of reactants...

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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?
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
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?
Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr, respectively, were allowed to react at 300. K. At equilibrium the total pressure was 110.5 torr. The reaction is 2NO(g)+Br2(g)2NOBr(g) a. Calculate the value of Kp. b. What would be the partial pressures of all species if NO and Br2, both at an initial partial pressure of 0.30 atm, were allowed to come to equilibrium at this temperature?
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
Suppose 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?
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
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.
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
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.