Consider a stoppered flask containing benzene, iodine, and air which has reached equilibrium at 298 K. Which one of the following statements concerning the system at equilibrium is true? a) The pressure of the vapour phase is not constant. b) Evaporation of the liquid continues. O c) The colour of the licid phase will change d) The mass of solid iodine is not constant

Consider a stoppered flask containing benzene, iodine, and air which has reached equilibrium at 298 K. Which one of the following statements concerning the system at equilibrium is true? a) The pressure of the vapour phase is not constant. b) Evaporation of the liquid continues. O c) The colour of the licid phase will change d) The mass of solid iodine is not constant

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 5.3E: Which system in each pair best represents equilibrium species under standard conditions of...

See similar textbooks

Similar questions

Fill in the blanks: (a) At equilibrium, G is. (b) For C6H6(l)C6H6(g),H is. (+,,0) (c) When a pure solid melts, the temperature at which liquid and solid are in equilibrium and G=0 is called.
Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
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?
A mixture of benzene and toluene forms an ideal solution. The partial pressure for benzene and toluene at 27 C are 24.65 torr and 16.48 torr, respectively. Calculate the mole fraction of toluene vapour in equilibrium.
A mixture consiting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What are the equilibrium concentrations for all substances?
The equilibrium constant for dissociation of dinitrogen tetroxideN2O4(g) ↔ 2 NO2(g)is KP = 0.308763 at 298.0 KIf the total equilibrium pressure at 298.0 K is 0.86 bar, what is the partial pressure of NO2(g)?
The equilibrium constant for the gas-phase isomerization of borneol, C10H17OH, to isoborneol at 503 K is 0.106. A mixture consisting of 6.70 g of borneol and 12 .5 g of isoborneol in a container of volume 5.0 dm3 is heated to 503 K and allowed to come to equilibrium. Calculate the mole fractionsof the two substances at equilibrium.
The phase diagram for SO2 is shown here. (a) What doesthis diagram tell you about the enthalpy change in thereaction SO2(l) ---->SO2(g)? (b) Calculate the equilibriumconstant for this reaction at 100 °C and at 0 °C.(c) Why is it not possible to calculate an equilibrium constantbetween the gas and liquid phases in the supercriticalregion? (d) At which of the three points marked in reddoes SO2(g) most closely approach ideal-gas behavior?(e) At which of the three red points does SO2(g) behaveleast ideally?
When equal amounts of hydrogen, H2, and iodine, I2, are mixed together at a total pressure of 1 bar, the partial pressure of hydrogen iodide, HI, vapour produced from by the reaction H2(g) + I2(g) ⇌ 2 HI(g) is 22.8 kPa. Calculate the equilibrium constant for the reaction.
Explain the Criterion for chemical equilibrium for a fixed mass at a specified temperature and pressure ?
A mixture consisting of 1.000 mol H2O(g) and 1.000 mol CO(g) is placed ina reaction vessel of volume 10.00 L at 800. K. At equilibrium, 0.665 mol CO2(g) is present as a result of the reaction CO (g) + H2O (g)⇋ CO2(g)+H2(g). What is the value of Kp at 800 K?