Indicale whether each of the following equilibrium mixtures contains mostly products or mostly reactants:
a.
b.
c.
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Basic Chemistry
- The 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_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_forwardFor the following endothermic reaction at equilibrium: 2SO3(g)2SO2(g)+O2(g) which of the following changes will increase the value of K? a. increasing the temperature b. decreasing the temperature c. removing SO3(g) (constant T) d. decreasing the volume (constant T) e. adding Ne(g) (constant T) f. adding SO2(g) (constant T) g. adding a catalyst (constant T)arrow_forward
- . Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a closed vessel according to the equation H2O(g)+CO(g)H2(g)+CO2(g)a. You add more H2O to the flask. How does the new equilibrium concentration of each chemical compare to its origin al equilibrium concentration after equilibrium is re-established? Justify your answer. b. You add more H2to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.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_forwardPhosphorus pentachloride decomposes at elevated temperatures. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 3.120 g of PCl5, 3.845 g of PCl3, and 1.787 g of Cl2 in a 10.0-L flask. If you add 1.418 g of Cl2, how will the equilibrium be affected? What will the concentrations of PCl5, PCl3, and Cl2 be when equilibrium is reestablished?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_forwardConsider the following hypothetical dissociation: AB3(s) A3+(aq)+3 B(aq)H0What effect will each of the following have on the position of equilibrium? (a) addition of A(NO3)3 (b) increase in temperature (c) adding Na+, forming NaBarrow_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
- Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forwardKp for the formation of phosgene, COCl2, is 6.5 1011 at 25 C. CO(g) + Cl2(g) COCl2(g) What is the value of Kp for the dissociation of phosgene? COCl2(g) CO(g) + Cl2(g)arrow_forwardThe decomposition of NH4HS, NH 4 HS( s )NH3( g )+ H 2 S( g ) is an endothermic process. Using Le Chatelier's 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_forward
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