The following pictures represent the equilibrium mixtures of five different chemical reactions. All the reactions proceed according to the general balanced chemical reaction A+B=AB Red spheres represent A atoms, blue spheres are B atoms, and red-blue clusters are AB molecules. Rank the reactions in order of increasing equilibrium constant. Rank the reactions from smallest to largest equilibrium constant To rank items as equivalent, overlap them. ► View Available Hint(s) Smallest equilibrium constant The correct ranking cannot be determined. Reset Help Largest equilibrium constant

The following pictures represent the equilibrium mixtures of five different chemical reactions. All the reactions proceed according to the general balanced chemical reaction A+B=AB Red spheres represent A atoms, blue spheres are B atoms, and red-blue clusters are AB molecules. Rank the reactions in order of increasing equilibrium constant. Rank the reactions from smallest to largest equilibrium constant To rank items as equivalent, overlap them. ► View Available Hint(s) Smallest equilibrium constant The correct ranking cannot be determined. Reset Help Largest equilibrium constant

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Given the reaction: ½ N₂O4(g) --> <-- NO2(g) The equilibrium constant is given as 3.3 at 373K. The value of the equilibrium constant will change if: (1) the partial pressures are given instead of concentrations (2) the temperature is increased to 473K (3) the concentration of the reactant is doubled. 1 and 2 only 1, 2 and 3 2 and 3 only 1 only 2 only M
(11 Try Again Your answer is incorrect. • reaction vessel C: Your answer is incorrect. A chemical engineer is studying the following reaction: BF3(aq) + NH3(aq) → BF3NH3(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.63. с The engineer charges ("fills") three reaction vessels with boron trifluoride and ammonia, and lets the reaction begin. He then measures the composition of the mixture inside 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. reaction vessel A B compound BF 3 NH3 BF₂NH₂ BF 3 NH₂ BF₂NH3 concentration 0.47 M 0.48 M 1.03 M 0.46 M 0.47 M 1.04 M expected change in concentration ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↓ decrease ↓ decrease O decrease ↓ decrease ↓ decrease decrease (no change) (no change) (no change) (no change) (no change) (no change)
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consider the following equilibrium reaction and how it might shift with each listed change. Write down your predictions and your reasoning for each. Fe3+ (aq) + SCN- (aq) < -- > Fe(SCN)2+ (aq) 1) add Fe(NO3)3 2) add KSCN 3) add NH4CL 4) add AgNO3 5) make it cold 6) make it hot
Two chemical reactions illustrated in sample A and sample B are set up with the starting materials shown at t = 0 s. The composition of the sample is checked 5 s later to determine the new distribution of reactants and products. Write an equilibrium equation for the reaction that is occurring. Using the models provided, which sample is most likely at equilibrium? Use only the information provided to draw your conclusion. Choose one or more:Sample ASample BNeither sample is at equilibrium. Which is true regarding the equilibrium constant? Choose one or more:A.The constant is 0.B.The constant is less than 1.C.The constant is greater than 1.
For this reaction: 2CO2(g) 2CO(2) + O2(e) Kequals 2.35 x 10Pat a particular temperature. If 3.5 moles of CO2 are initially placed into a 3.0L flask, calculate the equilibrium concentrations of all species. YOU MUST SHOW ALL OF YOUR WORK. | Drag n' Drop here or Browse Next
Consider the following system at equilibrium: P(aq) + Q(aq) = 3R(aq) Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help Decrease [R] Decrease [Q] Increase [P] Decrease [P] Triple [P] and reduce [Q] to one third Increase [R] Triple both [Q] and [R] Increase [Q] Leftward shift Rightward shift No shift
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AutoSave CHEM 212 Final Exam_Fall 2020 Word Search 困 ff steve M SM File Home Insert Draw Design Layout References Mailings Review View Help E Share O Comments 3a) Calculate AGon for this reaction: CH3OH (g) → CO (g) + 2 H2 (g) The equilibrium partial pressures for each component are: CH;OH = 0.620 atm, CO = 0.105 atm, H2 = 0.125 atm b) Is the reaction spontaneous? Briefly explain. 3c) Cells use the hydrolysis of adenosine triphosphate (ATP) as a source of energy. The conversion of ATP to ADP has a standard free energy change of -30.5 kJ/mol. If all the free energy from the metabolism of glucose goes to the conversion of ADP to ATP, how many mole of ATP can be produced for each mole of glucose? Page 3 of 6 492 words D Focus 80%
Writing the concentration equilibrium expression for a.. Write the concentration equilibrium constant expression for this reaction. CH3CO,H(aq)+C,H,OH(aq)→CH;CO,C,H,(aq)+H,0(1)
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 6.1 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 3.7 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. Check Explanation Access O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy MAR 28 MacBook Air