18. When 1 mole of ethene in the gas state reacts with 1 mole of water in the gas state, 1 mole of ethanol in the gas state is produced in an equilibrium reaction. If an equilibrium mixture contains 0.020 M ethene and 0.015 M water, the equilibrium concentration of ethanol is 1.35 M. The equilibrium constant for this reaction is 9000. (True or False)

18. When 1 mole of ethene in the gas state reacts with 1 mole of water in the gas state, 1 mole of ethanol in the gas state is produced in an equilibrium reaction. If an equilibrium mixture contains 0.020 M ethene and 0.015 M water, the equilibrium concentration of ethanol is 1.35 M. The equilibrium constant for this reaction is 9000. (True or False)

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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Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed? a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases
1) When a system is at equilibrium: A) the reaction rate of the forward reaction is equal to the rate of the reverse B) the reaction rate of the reverse reaction is small compared to forward C) the reaction rate of the forward reaction is small compared to the reverse D) the amount of product and reactant is exactly equal 2) What will be the equilibrium expression for this reaction? (DO NOT INCLUDE SOLID PRODUCTS, THEIR CONCENTRATION IS ALWAYS EQUAL TO 1.) 4 CuO (s) + CH4 (g) = CO2 (g)+ 4 Cu (s) + 2 H2O (g) A) [CuO]/[Cu] B) [CuO]4/[Cu]4 C) [Cu]4/[CuO]4 D) [CO2][H20]2/[CH4] 3) Which K value below corresponds to the system with the highest proportion of reactants? А) К 3D25 B) K = 0.067 C) K = 1.5 x 10-3 D) K 3D 1.2 х 103
Ammonia has been studied as an alternative "clean" fuel for internal combustion engines, since its reaction with oxygen produces only nitrogen and water vapor, and in the liquid form it is easily transported. An industrial chemist studying this reaction fills a 25.0 L tank with 1.5 mol of ammonia gas and 2.4 mol of oxygen gas, and when the mixture has come to equilibrium measures the amount of nitrogen gas to be 0.60 mol. Calculate the concentration equilibrium constant for the combustion of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K_ = ] |x10 ?
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O KINETICS AND EQUILIBRIUM Calculating an equilibrium constant from a partial equilibrium... 0/5 Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 21. mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.3 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. K = 0 II
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