(a)
Interpretation: The reaction of decomposition of
Concept introduction: The state when the reactants involved in a
According to Le Chatelier’s principle “When equilibrium is subjected to change in variable, the shift in the equilibrium is produced in the direction that nullifies the effect of change.”
To determine: The shift of equilibrium for the given reaction when
(b)
Interpretation: The reaction of decomposition of
Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.
According to Le Chatelier’s principle “When equilibrium is subjected to change in variable, the shift in the equilibrium is produced in the direction that nullifies the effect of change.”
To determine: The shift of equilibrium for the given reaction when
(c)
Interpretation: The reaction of decomposition of
Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.
According to Le Chatelier’s principle “When equilibrium is subjected to change in variable, the shift in the equilibrium is produced in the direction that nullifies the effect of change.”
To determine: The shift of equilibrium for the given reaction when
(d)
Interpretation: The reaction of decomposition of
Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.
According to Le Chatelier’s principle “When equilibrium is subjected to change in variable, the shift in the equilibrium is produced in the direction that nullifies the effect of change.”
To determine: The shift of equilibrium for the given reaction when argon gas is added.
(e)
Interpretation: The reaction of decomposition of
Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.
According to Le Chatelier’s principle “When equilibrium is subjected to change in variable, the shift in the equilibrium is produced in the direction that nullifies the effect of change.”
To determine: The shift of equilibrium for the given reaction when volume of reaction is doubled.
(f)
Interpretation: The reaction of decomposition of
Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.
According to Le Chatelier’s principle “When equilibrium is subjected to change in variable, the shift in the equilibrium is produced in the direction that nullifies the effect of change.”
To determine: The shift of equilibrium when temperature is decreased (exothermic reaction) for the given reaction.
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Chemistry: An Atoms First Approach
- What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?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_forwardConsider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species. (b) The volume of the container is decreased to 4.5 L and the system allowed to return to equilibrium. Calculate the new equilibrium concentrations. (Hint: The calculation will be easier if you view this as a new problem with 0.5 mol of COBr2 transferred to a 4.5-L flask.) (c) What is the effect of decreasing the container volume from 9.50 L to 4.50 L?arrow_forward
- Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?arrow_forwardA solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.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_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_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_forwardFor the equilibrium 2 SO2(g) + O2(g) 2 SO3(g) Kc = 245 (at 1000 K) the equilibrium concentrations are [SO2] = 0.102, [O2] = 0.0132, and [SO3] = 0.184. The concentration of SO2 is suddenly doubled. Show that the forward reaction takes place to reach a new equilibrium.arrow_forward
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