Please I need help eriment 14 - Google Chromeoodle.lsua.edu/mod/quiz/attempt.php?attempt=D1111199&cmid%=831398UA LSUA-EXANDRIAU b. Shift to the letO. No shiftO d. shift to the rightsestion 4If the pressure was decreased for the following reaction that was at equilibrium, how will the equilibrium position shift?ot yetN2(g) + O2(g) <=> 2NO(g)sweredints out ofSelect one:O a. RightFlag questionO b. No ShiftO. GasexO d. Cannot determineO e. Leftuestion 5Predict how the equilibrium position will shift if 100 grams of NaSCN is added to a solution containing the following at equilibrium?ot yetnsweredFe (aq) + SCN'(aq) <=> FESCN²*(aq)pints out ofL00Select one:- Flag questionO a. No shiftO b. shift to the leftO. shift to the rightO d. Cannot determinerMCCA TODELLFCDIIF1prt scF2F3F4F5F6F7F8F9F10

Answered: Image /qna-images/answer/d5ec180a-7e2a-4098-a6db-bee4e8ff3ac7.jpg

If the pressure was decreased for the following reaction that was at equilibrium, how will the equilibrium position shift? N2(g) + Oz(g) <=> 2NO(g) Select one: O a. Right tion O b. No Shift Gasex O d. Cannot determine O e. Left Predict how the equilibrium position will shift if 100 grams of NaSCN is added to a solution containing the following at equilibrium? Fe*(aq) + SCN (aq) <=> FESCN? (aq) Select one: No shift stion O b. shift to the left O. shift to the right O d. Cannot determine

If the pressure was decreased for the following reaction that was at equilibrium, how will the equilibrium position shift? N2(g) + Oz(g) <=> 2NO(g) Select one: O a. Right tion O b. No Shift Gasex O d. Cannot determine O e. Left Predict how the equilibrium position will shift if 100 grams of NaSCN is added to a solution containing the following at equilibrium? Fe*(aq) + SCN (aq) <=> FESCN? (aq) Select one: No shift stion O b. shift to the left O. shift to the right O d. Cannot determine

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 9RQ: What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at...

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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?
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?
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Iodine chloride decomposes at high temperatures to iodine and chlorine gases. 2ICl(g)I2(g)+Cl2(g)Equilibrium is established at a certain temperature when the partial pressures of ICl, I2, and Cl2 are (in atm) 0.43, 0.16, and 0.27, respectively. (a) Calculate K. (b) If enough iodine condenses to decrease its partial pressure to 0.10 atm, in which direction will the reaction proceed? What is the partial pressure of iodine when equilibrium is reestablished?
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
. 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?
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
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?
. For the reaction 2H2O(g)2H2(g)+O2(g)K=2.4103at a given temperature. At equilibrium ills found that [H2O(g)]=1.1101Mand [H2(g)]=1.9102M. What is the concentration of O2(g) under these conditions?
. Write the equilibrium expression for each of the following heterogeneous equilibria. a. 4Al(s)+3O2(g)2Al2O3(s)b. NH3(g)+HCl(g)NH4Cl(s)C. 2Mg(s)+O2(g)2MgO(s)