Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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demonstrate an understanding of the concept of dynamic equilibrium and the variables that cause shifts in the equilibrium of chemical systems.
Transcribed Image Text:1.
You are a chemical engineer that is responsible for synthesizing a new drug. You
look at a series of potential chemical reactions that will make your drug along with
their respective K values. What type of K value would you be looking for and why?
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- While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene (CH,CH,) with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a 100 L tank with 45. mol of ethylene gas and 35. mol of water vapor. When the mixture has come to equilibrium he determines that it contains 34. mol of ethylene gas and 24. mol of water vapor. The engineer then adds another 18. mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of ethanol after equilibrium is reached the second time. Round your answer to 2 significant digits. | molarrow_forwardTrue/False. Explain your answer in one sentence or less. In an equilibrium process, the concentrations of products and of reactants are equal. The value of the equilibrium constant for a given reaction depends on the initial concentrations of reactants. Large value for equilibrium constant K means the reaction will be less complete at the equilibrium point. The concentration of a pure solid is left out of an equilibrium constant expression but a pure liquid is included.arrow_forwardConsider the equilibrium system described by the chemical reactionbelow. Calculate the value of Qc for the initial set reaction conditions in3.00 L container:8.65 g C2H4, 11.2 g O2, and 5.68 g CH3CHO. 2 C2H4(g) + O2(g) = 2 CH3CHO(g)arrow_forward
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