(a) Determine whether the value of K of an equilibrium system will be affected or,unaffected by the following changes:ChangesValue of K(affected or unaffected)(O Decreasing the temperature(1) Increasing the pressure of the system() Decreasing the concentration of reactant(b) The following graph represents the amount of CO formed at two different temperatures,T; and T. The reaction as shown below:C() + H,O(g) = co(g) + H(g)T = 385 K[co)T = 335 KtimeBased on the graph, determine whether the forward reaction is endothermic orexothermic.Predict if the concentration of H:0 gas increases, decreases or remains the sameif the temperature is decreased to 298 K. Explain.A mixture of 0.350 M of H:0, 0.125 M of CO and 0.125 M of H: was preparedand allowed to reach equilibrium in a 1.00 L flask. The equilibriumconcentration of H;0 is 0.182 M. Calculate the Ke of the reaction at constanttemperature.(H)

Answered: Image /qna-images/answer/f8e48f0b-4320-4a92-8691-d6828077ca01.jpg

(a) Determine whether the value of K of an equilibrium system will be affected or unaffected by the following changes: Changes Value of K (affected or unaffected) (Decreasing the temperature (u) Increasing the pressure of the system (uD Decreasing the concentration of reactant (b) The following graph represents the amount of CO formed at two different temperatures, and Ts. The reaction as shown below: Cts) + H,O(g) = Co(g) + H:(g) T 385 K T = 335 K time Based on the graph, determine whether the forward reaction is endothermic or exothermic. Predict if the concentration of H.O gas increases, decreases or remains the same if the temperature is decreased to 298 K. Explain. A mixture of 0.350 M of H:0, 0.125 M of CO and 0.125 M of H: was prepared and allowed to reach equilibrium in a 1.00 L flask. The equilibrium concentration of H:0 is 0.182 M. Calculate the Ke of the reaction at constant: temperature.

(a) Determine whether the value of K of an equilibrium system will be affected or unaffected by the following changes: Changes Value of K (affected or unaffected) (Decreasing the temperature (u) Increasing the pressure of the system (uD Decreasing the concentration of reactant (b) The following graph represents the amount of CO formed at two different temperatures, and Ts. The reaction as shown below: Cts) + H,O(g) = Co(g) + H:(g) T 385 K T = 335 K time Based on the graph, determine whether the forward reaction is endothermic or exothermic. Predict if the concentration of H.O gas increases, decreases or remains the same if the temperature is decreased to 298 K. Explain. A mixture of 0.350 M of H:0, 0.125 M of CO and 0.125 M of H: was prepared and allowed to reach equilibrium in a 1.00 L flask. The equilibrium concentration of H:0 is 0.182 M. Calculate the Ke of the reaction at constant: temperature.

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 123CP: A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless,...

See similar textbooks

Similar questions

Write the equilibrium constant expression for each reaction in terms of activities, simplifying where appropriate. a C(s)+O2(g)CO2(g) b P4(s)+5O2(g)P4O10(s) c 2HNO2(g)+3Cl2(g)2NCl3(g)+H2(g)+2O2(g)
For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?
For the following reactions, predict whether the pressure of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. (a) H2O(l)H2O(g) (b) N2(g)+3H2(g)2NH3(g) (c) C2H4(g)+H2O(g)C2H5OH(g)
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?
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?
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?
Hydrogen, bromine, and HBr in the gas phase are in equilibrium in a container of fixed volume. H2(g) + Br2(g) 2 HBr(g) rH = 103.7 kJ/mol How will each of these changes affect the indicated quantities? Write increase, decrease, or no change.
Mustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?
. 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.
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.
. 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?
Draw a nanoscale (particulate) level diagram for an equilibrium mixture of