Using an equilibrium constant to predict the direction of spontaneous...A chemical engineer is studying the following reaction:H2(g)+I2(g) →2 HI(g)Press (fn) F to exit full screen1/3At the temperature the engineer picks, the equilibrium constant ✓ for this reaction is 0.50.РThe engineer charges ("fills") three reaction vessels with hydrogen and iodine, and lets the reaction begin. He then measures the composition of the mixtureinside each vessel from time to time. His first set of measurements are shown in the table below.Predict the changes in the compositions the engineer should expect next time he measures the compositions.reactionvesselcompoundpressureexpected change in pressureH23.13 atm↑ increase↓ decrease(no change)A123.72 atm↑ increase↓ decrease(no change)HI1.26 atm↑ increase↓ decrease(no change)H22.22 atm↑ increase↓ decrease(no change)BI,2.81 atm↑ increase↓ decrease(no change)HI3.06 atm↑ increase↓ decrease(no change)H₁2.70 atm↑ increase↓ decrease(no change)C123.29 atm↑ increase↓ decrease(no change)HI2.11 atm↑ increase↓ decrease(no change)

To predict the changes in the composition of the mixtures in each reaction vessel, we need to…

Answered: Using an equilibrium constant to…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 69QAP: Consider the reaction: A(g)+2B(g)+C(s)2D(g)At 25C, only A, B, and C are present. The partial...

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Similar questions

The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.
The atmosphere consists of about 80% N2 and 20% O2, yet there are many oxides of nitrogen that are stable and can be isolated in the laboratory. (a) Is the atmosphere at chemical equilibrium with respect to forming NO? (b) If not, why doesnt NO form? If so, how is it that NO can be made and kept in the laboratory for long periods?
The equilibrium constant for a certain reaction decreases from 8.84 to 3.25 102 when the temperature increases from 25C to 75C. Estimate the temperature where K = 1.00 for this reaction. Estimate the value of S for this reaction. (Hint: Manipulate the equation in Exercise 79.)
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?
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?
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
. Gaseous phosphorus pentachloride decomposes according to the reaction PCl5(g)PCl3(g)+Cl2(g)The equilibrium system was analyzed at a particular temperature, and the concentrations of the substances present were determined to be [PCl5]=1.1102M,[PCl3]=0.325M. and [Cl2]=3.9103M. Calculate the value of K for the reaction.
5.12. True or false: If all the partial pressures of reactants and products drop by half, the value of Q drops by half. Give an example of a chemical reaction to support your answer.
Consider the reaction: A(g)+2B(g)+C(s)2D(g)At 25C, only A, B, and C are present. The partial pressures of A, B, and D are given as PA, PB, and PD. Equilibrium is established 18 minutes after the reaction starts. Use terms is less than (LT), is greater than (GT), is equal to (EQ), or insufficient information (X) to answer the following questions. (a) PD at 5 min PA. (b) PA at 21 min PA at 27 min. (c) PB at 7 min PB at 13 min.(d) After 20 min, more B is added. When equilibrium is reestablished, K before the addition K after the addition. (e) After 20 min, the temperature is increased to 35C. PA before the temperature increase PA after the temperature increase after equilibrium is reestablished.
Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant expression for the reaction. Call the equilibrium constant K1. (b) Write an equilibrium constant expression for the formation of one mole of B(g) and call the equilibrium constant K2. (c) Relate K1 and K2.
Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial pressure of CO2 at room temperature?
In Table 12.1 (←Sec. 12-3a) the equilibrium constant for the reaction ⇋ is given as 4.2 × 1052. If this reaction is so product-favored, why can large piles of yellow sulfur exist in our environment (as they do in Louisiana and Texas)?

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