b ASd) H₂(g) + 1₂ (g) = 2 HI(g) is @equilibriumWAven thisspoPredict the cause of each stress as I = increase,D-decrease or N=no change1) when HI is added, the4329ont toIt shH₂quzizim 21 streams2) when H₂ is removed from the vessel,the amount of Iz will590es10)3) When the volume of the vessel isdoubled, K willele Aeo17 A

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d) H₂(g) + 1₂ (g) = 2 HI(g) is @equilibrium When thiso; bus spo Predict the cause of each stress as I = increase, D-decrease or N=no changezeshaje pist+ 1) When HI is added, the amount of H₂ will it to 2) when H₂ is removed from the vessel, the amount of Iz will d 3) when the volume of the vessel is doubled, K will. ale Aeo17

d) H₂(g) + 1₂ (g) = 2 HI(g) is @equilibrium When thiso; bus spo Predict the cause of each stress as I = increase, D-decrease or N=no changezeshaje pist+ 1) When HI is added, the amount of H₂ will it to 2) when H₂ is removed from the vessel, the amount of Iz will d 3) when the volume of the vessel is doubled, K will. ale Aeo17

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 118CP: Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain...

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For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture consists of all three gases with the following partial pressures: PPCl5=0.026atm,PPCl3=0.65atmPPCl2=0.33atm (a) Is the system at equilibrium? Explain. (b) If the system is not at equilibrium, in which direction will the system move to reach equilibrium?
A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure at equilibrium is 40% greater than it was originally, when only I2 was present. What is K for this reaction at that temperature?
. The reaction C2H2(g)+2Br2(g)C2H2Br4(g)is exothermic in the forward direction. Will an increase in temperature shift the position of the equilibrium toward reactants or products?
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer
Explain how to recognize the conditions under which changes in pressure would affect systems at equilibrium.
At 2000 K, experiments show that the equilibrium constant for the formation of water is 1.6 1010. 2H2(g) + O2(g) 2H2O(g) Calculate the equilibrium constant at the same temperature for H2(g)+12O2(g) H2O(g)
The figures below represent the following reaction at equilibrium at different temperatures. A2(g)+3B2(g)2AB3(g)where squares represent atom A and circles represent atom B. Is the reaction exothermic?
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.
Suppose a reaction has the equilibrium constant K = 1.7 108 at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?
Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
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?
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?