CHAPTER 7 - GASES, LIQUIDS, AND SOLIDS O Previous Page 14 of 36 Next O A mass of 1.36 g of an unknown gas exerts a pressure of 0.790 atm at 71°C in a 1.00-L flask. What is the molar mass of the gas? (R =0.08206 L-atm/mol-K O Previous Page 13 of 36 Next O What is the pressure exerted by 1.39 g Xe gas at 17.0 'C in a 340-mL flask?

CHAPTER 7 - GASES, LIQUIDS, AND SOLIDS O Previous Page 14 of 36 Next O A mass of 1.36 g of an unknown gas exerts a pressure of 0.790 atm at 71°C in a 1.00-L flask. What is the molar mass of the gas? (R =0.08206 L-atm/mol-K O Previous Page 13 of 36 Next O What is the pressure exerted by 1.39 g Xe gas at 17.0 'C in a 340-mL flask?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter13: Fundamental Equilibrium Concepts

Section: Chapter Questions

Problem 61E: Complete the changes in concentrations (or pressure, if requested) for each of the following...

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A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g)X(g)+Y(g) A 2.00-g sample of XY (molar mass = 165 g/mol) is placed in a container with a movable piston at 25C. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until 35.0 mole percent of the original XY has dissociated and then remains at a constant position. Assuming ideal behavior, calculate the density of the gas in the container after the piston has stopped moving, and determine the value of K for this reaction of 25C.
The graph below is similar to that of Figure 12.2. If after 100 s have elapsed the partial pressure of N2O4 is increased to 1.0 atm, what will the graph for N2O4 look like beyond 100 s?
A chemist wants to prepare phosgene, COCl2, by the following reaction: CO(g)+Cl2(g)COCl2(g) He places 4.00 g of chlorine, Cl2, and an equal molar amount of carbon monoxide, CO, into a 10.00-L reaction vessel at 395C. After the reaction comes to equilibrium, he adds another 4.00 g of chlorine to the vessel in order to push the reaction to the right to get more product. What is the partial pressure of phosgene when the reaction again comes to equilibrium? Kc = 1.23 103.
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
Complete the changes in concentrations (or pressure, if requested) for each of the following reactions‘ (a) 2H2(g)+O2(g)2H2O(g) + 2x 1.50M (b) CS2(g)+4H2(g)CH4(g)+2H2S(g) x 0.020 M (c) Change in pressure: H2(g)+CI2(g)2HCI(g)x 1.50 atm (d) Change in pressure: 2NH3(g)+2O2(g)N2O(g)+3H2O(g) x = 60.6 torr (e) NH4HS(s)NH3+H2S(g) x 9.8106M (f) Change in pressure: Fe(s)+5CO(g)Fe(CO)5(g) x 0.012 atm
Ammonium hydrogen sulfide. NH4HS, is unstable at room temperature and decomposes: NH4HS(s)NH3(g)+H2S(g) You have placed some solid ammonium hydrogen sulfide in a closed flask. Which of the following would produce less hydrogen sulfide, H2S, which is a poisonous gas? a Removing some NH3 from the flask b Adding some NH3 to the flask c Removing some of the NH4HS d Increasing the pressure in the flask by adding helium gas
Consider a cylinder containing a mixture of liquid carbon dioxide in equilibrium with gaseous carbon dioxide at an initial pressure of 65 atm and a temperature of 20 C. Sketch a plot depicting the change in the cylinder pressure with time as gaseous carbon dioxide is released at constant temperature.
. Equilibrium is microscopically dynamic but macroscopically static. Explain what this means.
The partial pressures of an equilibrium mixture of N2O4(g) and NO2(g) are PN2O4=0.34 atm and PNO2=1.20 atm at a certain temperature. The volume of the container is doubled. Calculate the partial pressures of the two gases when a new equilibrium is established.
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?
Consider the equilibrium process depicted in Fig. 17.6. When does the equilibrium state occur?