Carbon dioxide and water react to form methanol and oxygen, like this: 2 CO,(9)+4 H,0(9)→2 CH,OH()+3 O,(9) At a certain temperature, a chemist finds that a 4.6 L reaction vessel containing a mixture of carbon dioxide, water, methanol, and axygen at equilibrium has the following composition: compound amount CO, 3.94 g H,0 4.50 g CH,OH 3.68 g 2.67 8 Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ - 0 Explanation Check 2022 MeGraw H LLC A Rights Reserved Terms of Use Pvacy Center Accessibty pe here to search (99+

Carbon dioxide and water react to form methanol and oxygen, like this: 2 CO,(9)+4 H,0(9)→2 CH,OH()+3 O,(9) At a certain temperature, a chemist finds that a 4.6 L reaction vessel containing a mixture of carbon dioxide, water, methanol, and axygen at equilibrium has the following composition: compound amount CO, 3.94 g H,0 4.50 g CH,OH 3.68 g 2.67 8 Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ - 0 Explanation Check 2022 MeGraw H LLC A Rights Reserved Terms of Use Pvacy Center Accessibty pe here to search (99+

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 3RQ

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Similar questions

At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
A 4.72-g sample of methanol (CH3OH) was placed in an otherwise empty 1.00-L flask and heated to 250.C to vaporize the methanol. Over time, the methanol vapor decomposed by the following reaction: CH3OH(g)CO(g)+2H2(g) After the system has reached equilibrium, a tiny hole is drilled in the side of the flask allowing gaseous compounds to effuse out of the flask. Measurements of the effusing gas show that it contains 33.0 times as much H2(g) as CH3OH(g). Calculate K for this reaction at 250.C.
Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a product
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
For the system PCl5(g)PCl3(g)+Cl2(g)K is 26 at 300C. In a 1.0-L flask at 300C, a gaseous mixture consists of all three gases with the following partial pressures: PPCl5=0.026atm,PPCl3=0.65atmPPCl2=0.33atm (a) Is the system at equilibrium? Explain. (b) If the system is not at equilibrium, in which direction will the system move to reach equilibrium?
5.2. What is the difference between a static equilibrium and a dynamic equilibrium? Give examples difference from the examples in the text. What is similar for the two types of equilibria?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.

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