Methanol can be prepared from carbon monoxide and hydrogen at high temperature and pressure in the presence of a suitable catalyst according to the followingequation:2H2(g) + CO(g)= CH3OH(g) AH=-90.2kJThe reaction is at equilibrium and cO is removed. After this removal, the concentration of Hand the concentration of CH3OHdecreasesto reestablish equilibrium.increasesdoes not change

The equilibrium constant represents the concentration of the products and the concentration of the…

ethanol can be prepared from carbon monoxide and hydrogen at high temperature and pressure in the presence of a suitable catalyst according to t quation: H2(g) + CO(g) = CH3OH(g) AH=-90.2kJ he reaction is at equilibrium and CO is removed. After this removal, the concentration of HV A and the concentration of CH3OH decreases to reestablish equilibrium. increases does not change

ethanol can be prepared from carbon monoxide and hydrogen at high temperature and pressure in the presence of a suitable catalyst according to t quation: H2(g) + CO(g) = CH3OH(g) AH=-90.2kJ he reaction is at equilibrium and CO is removed. After this removal, the concentration of HV A and the concentration of CH3OH decreases to reestablish equilibrium. increases does not change

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 118CP: Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain...

See similar textbooks

Similar questions

Isopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction: C3H7OH(g)C2H6CO(g)+H2(g)At 180C, the equilibrium constant for the decomposition is 0.45. If 20.0 mL (d=0.785g/mL) of isopropyl alcohol is placed in a 5.00-L vessel and heated to 180C, what percent- age remains undissociated at equilibrium?
Colorless N2O4 gas decomposes to form red-brown colored NO2 gas. Describe how the concentrations of N2O4 and NO2 would change increase or decrease as equilibrium was established in a sealed container that initially contained only N2O4. What observation would indicate that equilibrium had been established?
. Ammonia. a very important industrial chemical. is produced by the direct combination of the following elements under carefully controlled conditions: N2(g)+3H2(g)2NH3(g)Suppose. in an experiment, that the reaction mixture is analyzed after equilibrium is reached, and it is found, at a particular temperature. that [NH3]=0.25M,[H2]=3.4103M, and [N2]=5.3105M. Calculate the value of K at this temperature.
Benzaldehyde, a flavoring agent, is obtained by the dehydrogenation of benzyl alcohol. C6H5CH2OH(g)C6H5CHO(g)+H2(g)K for the reaction at 250C is 0.56. If 1.50 g of benzyl alcohol is placed in a 2.0-L flask and heated to 250C, (a) what is the partial pressure of the benzaldehyde when equilibrium is established? (b) how many grams of benzyl alcohol remain at equilibrium?
A 100.-gram sample of sodium chloride (NaCl) is added to 100. mL of water at 0 C. After equilibrium is reached, about 64 g of solid remains undissolved. Describe the equilibrium that exists in this system at the particulate level.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
For a typical equilibrium problem, the value of K and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?
. Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the inter-conversion reaction?
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure at equilibrium is 40% greater than it was originally, when only I2 was present. What is K for this reaction at that temperature?
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer