Course Contents » ... » Homework Set #4 » t10p18a Timer Notes Evaluate Feedback Print Info Given the following equilibrium system: 25O2(g) + 02(g) 2503(g) + 99.1 kJ If additional SO2(g) is added to the system while the temperature and pressure are kept constant. Compared to its original concentration, how will the concentration, of oxygen change? Decrease Increase Remain the Same Submit Answer Tries 0/99 The pressure on the system is increased while the temperature is kept constant. Compared to its original concentration, how will the concentration of SO2(g) change? Increase Decrease Remain the Same Submit Answer Tries 0/99 A catalyst is added to the above equilibrium system while the temperature and pressure are kept constant. Compared to its original concentration, how will the new equilibrium concentration of SO2(g) change? Increase Remain the Same Decrease Submit Answer Tries 0/99 The temperature of the equilibrium system is decreased and the pressure is kept constant. Compared to its orginal concentration, how will the new equilibrium concentration of SO2(g) change? Remain the Same Decrease Increase Submit Answer Tries 0/99 000 000 000

Course Contents » ... » Homework Set #4 » t10p18a Timer Notes Evaluate Feedback Print Info Given the following equilibrium system: 25O2(g) + 02(g) 2503(g) + 99.1 kJ If additional SO2(g) is added to the system while the temperature and pressure are kept constant. Compared to its original concentration, how will the concentration, of oxygen change? Decrease Increase Remain the Same Submit Answer Tries 0/99 The pressure on the system is increased while the temperature is kept constant. Compared to its original concentration, how will the concentration of SO2(g) change? Increase Decrease Remain the Same Submit Answer Tries 0/99 A catalyst is added to the above equilibrium system while the temperature and pressure are kept constant. Compared to its original concentration, how will the new equilibrium concentration of SO2(g) change? Increase Remain the Same Decrease Submit Answer Tries 0/99 The temperature of the equilibrium system is decreased and the pressure is kept constant. Compared to its orginal concentration, how will the new equilibrium concentration of SO2(g) change? Remain the Same Decrease Increase Submit Answer Tries 0/99 000 000 000

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter5: Introduction To Chemical Equilibrium

Section: Chapter Questions

Problem 5.16E: 5.16. In atmospheric chemistry, the following chemical reaction converts , the predominant oxide of...

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Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the equilibrium constant at 225°C is 6.08103. Assume that the ratio of the pressures of CO(g) and H2(g) is 1:2. What values should they have if the partial pressureof methanol is to be 0.500 atm?
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)
5.16. In atmospheric chemistry, the following chemical reaction converts , the predominant oxide of sulfur that comes from combustion of S-containing materials, to , which can combine with to make sulfuric acid (and thus contribute to acid rain): (a) Write the expression for K for this equilibrium. (b) Calculate the value of for this equilibrium using the values in Appendix 2. (c) Calculate the value of K for this equilibrium. (d) If of and of are enclosed in a system in the presence of some liquid, in which direction would the reaction move?
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
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
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?
. 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?
For the following system, K=4.86105 at 298K: HClO(aq)+F(aq)ClO(aq)+HF(aq) Assuming that you start with equal concentrations of HClO and F, and that no ClO or HF is initially present, which of the following best describes the equilibrium system: a the forward reaction is favored at equilibrium; b the reverse reaction is favored at equilibrium; c appreciable quantities of all species are present at equilibrium?
5.19. Assume that a reaction exists such that equilibrium occurs when the partial pressures of the reactants and products are all . If the volume of the system were doubled, all of the partial pressures would be . Would the system still be at equilibrium? Why or Why not?
. 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.
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?
12.85 In the figure, orange fish are placed in one aquarium and green fish in an adjoining aquarium. The two tanks are separated by a removable partition that is initially closed. Describe what happens in the first few minutes after the partition is opened. WTiat would you expect to see several hours later? How is this system analogous to dynamic chemical equilibrium?