The decomposition of
is an endothermic process. Using Le principle, explain how increasing the temperature would affect the equilibrium. If more
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- At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?arrow_forwardAt room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?arrow_forward12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.arrow_forward
- The decomposition of NH4HS NH4HS(s) NH3(g) + H2S(g) is an endothermic process. Using Le Chateliers principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which this equilibrium exists, how is the equilibrium affected? What if some additional NH3 is placed in the flask? What will happen to the pressure of NH3 if some H2S is removed from the flask?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_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_forward
- Two molecules of A react to form one molecule of B, as in the reaction 2 A(g) B(g) Three experiments are done at different temperatures and equilibrium concentrations are measured. For each experiment, calculate the equilibrium constant, Kc. (a) [A] = 0.74 mol/L, [B] = 0.74 mol/L (b) [A] = 2.0 mol/L, [B] = 2.0 mol/L (c) [A] = 0.01 mol/L, [B] = 0.01 mol/L What can you conclude about this statement: If the concentrations of reactants and products are equal, then the equilibrium constant is always 1.0.arrow_forwardThe equilibrium constant, Kc, is 1.05 at 350 K for the endothermic reaction 2 CH2Cl2(g) CH4(g) + CCl4(g) Which of the diagrams for Question 111 represents an equilibrium mixture at 350 K? Diagrams for Question 111.arrow_forwardSolid NH4HS decomposes by the following endothermic process: NH4HS(s) NH3(g) + H2S(g) a. What effect will adding more NH3(g) have on the equilibrium? b. What effect will adding more NH4HS(s) have on the equilibrium? c. What effect will increasing the volume of the container have on the equilibrium? d. What effect will decreasing the temperature have on the equilibrium?arrow_forward
- At 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. For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular temperature. a. What does the very small equilibrium constant indicate about the extent to which oxygen gas, O2(g), is converted to ozone gas, O3(g), at this temperature? b. If the equilibrium mixture is analyzed and [O2(g)]is found to be 3.04102M, what is the concentration of O3(g) in the mixture’?arrow_forwardThe reaction 2 NO2(g) N2O4(g) has an equilibrium constant, Kc, of 170 at 25 C. If 2.0 103 mol of NO2 is present in a 10.-L. Flask along with 1.5 103 mol of N2O4, is the system at equilibrium? If it is not at equilibrium, does the concentration of NO2 increase or decrease as the system proceeds to equilibrium?arrow_forward
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