Canvas POF SOU-CCJ230-Introd... Problem-Solving Strategies: Understanding Equilibrium▼ Part A Identify the stressConsider the equilibrium reactionCO(g) + H₂O(g) - CO₂(g) + H₂(g)Determine how each change in the left-hand column will stress the system and in which direction the equilibrium reaction will shift in response.Drag the appropriate labels to their respective targets.► View Available Hint(s)Increase reactantDecrease reactantIncrease productDecrease productSubmitType here to searchReverse reaction ratetemporarily increasesForward reaction ratetemporarily increasesForward reaction ratetemporarily decreasesReverse reaction ratetemporarily decreasesChangeAdd CO(g)Remove H₂O(g)Add CO₂(g)Remove H₂(g)IHSystem stressGroup 1Group 1Group 1Group 1✔CaEquilibrium shiftGroup 2Group 2Group 2Group 2ResetHelp

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em-Solving Strategies: Understanding Equilibrium For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g) + H₂O(1) NH₂ (aq) + OH-(aq) Drag the appropriate stresses to their respective bins. ► View Available Hint(s) Removing NH₂ (aq) Removing OH (aq) Shift in the direction of the reactants Adding OH (aq) Adding NH3(g) Adding NH₂ (aq) Shift in the direction of the products Reset Help

em-Solving Strategies: Understanding Equilibrium For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g) + H₂O(1) NH₂ (aq) + OH-(aq) Drag the appropriate stresses to their respective bins. ► View Available Hint(s) Removing NH₂ (aq) Removing OH (aq) Shift in the direction of the reactants Adding OH (aq) Adding NH3(g) Adding NH₂ (aq) Shift in the direction of the products Reset Help

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem 13STP

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Similar questions

The following series of diagrams represent the reaction XY followed over a period of time. The X molecules are red and the Y molecules are green. At the end of the time period depicted, has the reaction system reached equilibrium? Justify your answer with a one-sentence explanation.
Classify each of the following statements as true or false. aSome equilibria depend on a steady supply of a reactant in order to maintain the equilibrium. bBoth forward and reverse reactions continue after equilibrium is reached. cEvery time reactant molecules collide, there is a reaction. dPotential energy during a collision is greater than potential energy before or after the collision. eThe properties of a transition state are between those of the reactants and products. fActivation energy is positive for both the forward and reverse reactions. gKinetic energy is changed to potential energy during a collision. hAn increase in temperature speeds the forward reaction but slows the reverse reaction. iA catalyst changes the steps by which a reaction is completed. jAn increase in concentration of a substance on the right-hand side of an equation speeds the reverse reaction rate. kAn increase in the concentration of a substance in an equilibrium increases the reaction rate in which the substance is a product. lReducing the volume of a gaseous equilibrium shifts the equilibrium in the direction of fewer gaseous molecules. mRaising temperature results in a shift in the forward direction of an endothermic equilibrium. nThe value of an equilibrium constant depends on temperature. oA large K indicates that an equilibrium is favored in the reverse direction.
Characterize a system at chemical equilibrium with respect to each of the following a. the rates of the forward and reverse reactions b. the overall composition of the reaction mixture For a general reaction3A(g)+B(g)2C(g), if one starts an experiment with only reactants present, show what the plot of concentrations of A, B, and C versus time would look like. Also sketch the plot illustrating the rate of the forward reaction and rate of the reverse reaction versus time.
. In your own words, describe what Le Châtelier’s principle tells us about how we can change the position of a reaction system at equilibrium.
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?
How do chemists envision reactions taking place in terms of the collision model for reactions? Give an example of a simple reaction and how you might envision the reaction’s taking place by means of a collision between the molecules.
7-12 Two kinds of gas molecules are reacted at a set temperature. The gases are blown into the reaction vessel from two tubes. In setup A, the two tubes are aligned parallel to each other; in setup B, they are 900 to each other; and in setup C, they are aligned directly opposite each other. Which setup would yield the most effective collisions?