The following reaction is used self-contained breathing devices as a source of
Suppose that a sample of
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- Nitrosyl chloride, NOC1, decomposes to NO and Cl2 at high temperatures. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) Suppose you place 2.00 mol NOC1 in a 1.00–L flask, seal it, and raise the temperature to 462 °C. When equilibrium has been established, 0.66 mol NO is present. Calculate the equilibrium constant Kc for the decomposition reaction from these data.arrow_forwardDinitrogen tetroxide, N2O4, is a colorless gas (boiling point, 21C), which dissociates to give nitrogen dioxide, NO2 a reddish brown gas. N2O4(g)2NO2(g) The equilibrium constant Kc at 25C is 0.125. What percentage of dinitrogen tetroxidc is dissociated when 0.0400 mol N2O4 is placed in a 1.00-L flask at 25C?arrow_forwardPhosphorus pentachloride, PCl5, decomposes on heating to give phosphorus trichloride, PCl5, and chlorine. PCl5(g)PCl3(g)+Cl2(g) A closed 2.90-L vessel initially contains 0.0564 mol PCl5. What is the total pressure at 250C when equilibrium is achieved? The value of Kc at 250C is 4.15 102.arrow_forward
- Given K = 3.50 at 45C for the reaction A(g)+B(g)C(g) and K = 7.10 at 45C for the reaction 2A(g)+D(g)C(g) what is the value of K at the same temperature for the reaction C(g)+D(g)2B(g) What is the value of Kp, at 45c for the reaction? Starting with 1.50 atm partial pressures of both C and D, what is the mole fraction of B once equilibrium is reached?arrow_forwardGaseous acetic acid molecules have a certain tendency to form dimers. (A dimer is a molecule formed by the association of two identical, simpler molecules.) The equilibrium constant Kc at 25C for this reaction is 3.2 104. a If the initial concentration of CH3COOH monomer (the simpler molecule) is 4.0 104 M, what are the concentrations of monomer and dimer when the system comes to equilibrium? (The simpler quadratic equation is obtained by assuming that all of the acid molecules have dimerized and then some of it dissociates to monomer.) b Why do acetic acid molecules dimerize? What type of structure would you draw for the dimer? c As the temperature increases would you expect the percentage of dimer to increase or decrease? Why?arrow_forwardAt high temperatures, a dynamic equilibrium exists between carbon monoxide, carbon dioxide, and solid carbon. C(s)+CO2(g)2CO(g);H=172.5kJ At 850C, Kc is 0.153. a What is the value of Kp? b If the original reaction system consisted of just carbon and 1.50 atm of CO2, what are the pressures of CO2 and CO when equilibrium has been established? c How will the equilibrium pressure of CO change if the temperature is decreased?arrow_forward
- Gaseous acetic acid molecules have a certain tendency to form dimers. (A dimer is a molecules formed by the association of two identical, simpler molecules.) The equilibrium constant Kp at 25C for this reaction is 1.3 103. a If the initial pressure of CH3COOH monomer (the simpler molecule) is 7.5 103 atm, what are the pressures of monomer and dimer when the system comes to equilibrium? (The simpler quadratic equation is obtained by assuming that all of the acid molecules have dimerized and then some of it dissociates to monomer.) b Why do acetic acid molecules dimerize? What type of structure would you draw for the dimer? c As the temperature decreases, would you expect the percentage of dimer to increase or decrease? Why?arrow_forwardLexan is a plastic used to make compact discs, eyeglass lenses, and bullet-proof glass. One of the compounds used to make Lexan is phosgene (COCl2), an extremely poisonous gas. Phosgene decomposes by the reaction COCl2(g)CO(g)+Cl2(g) for which Kp 6.8 109 at 100C. If pure phosgene at an initial pressure of 1.0 atm decomposes, calculate the equilibrium pressures of all species.arrow_forwardKc for the decomposition of ammonium hydrogen sulfide is 1.8 104 at 25 C. NH4HS(s) NH3(g) + H2S(g) (a) When the pure salt decomposes in a flask, what are the equilibrium concentrations of NH3 and H2S? (b) If NH4HS is placed in a flask already containing 0.020 mol/L of NH3 and then the system is allowed to come to equilibrium, what are the equilibrium concentrations of NH3 and H2S?arrow_forward
- An equilibrium mixture of SO2, O2, and SO3 at a high temperature contains the gases at the following concentrations: |SO2| = 3.77 103 mol/L, [O2] = 4.30 103 mol/L, and [SO3] = 4.13 103 mol/L. Calculate the equilibrium constant, Kc, for the reaction. 2 SO2(g) + O2(g) 2 SO3(g)arrow_forwardA mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 5.0 103 mol/L, [O2] = 1.9 103 mol/L, and [SO3] = 6.9 103 mol/L. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? 2 SO2(g) + O2(g) 2 SO3(g) Kc = 279arrow_forwardCarbon dioxide reacts with carbon to give carbon monoxide according to the equation C(s)+CO2(g)2CO(g) At 700. C, a 2.0-L sealed flask at equilibrium contains 0.10 mol CO, 0.20 mol CO2, and 0.40 mol C. Calculate the equilibrium constant KP for this reaction at the specified temperature.arrow_forward
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