Interpretation:
Equilibrium reaction of
Concept Introduction:
Equilibrium constant
Equilibrium constant
Consider the reaction where A reacts to give B.
On rearranging,
Where,
Explanation of Solution
Given information,
Calculate the value of
Compare the value of
So the given reaction must proceeds toward reactants to reach equilibrium condition. So first take the reaction all the way to reactants as much as stoichiometrically possible, after that take it back to equilibrium with a very small x.
Construct ICE table,
At equilibrium,
Assume,
Solve for x,
Calculate the concentration of the substances,
Almost all the
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Chapter 12 Solutions
Chemistry: The Molecular Science
- 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_forwardThe atmosphere consists of about 80% N2 and 20% O2, yet there are many oxides of nitrogen that are stable and can be isolated in the laboratory. (a) Is the atmosphere at chemical equilibrium with respect to forming NO? (b) If not, why doesnt NO form? If so, how is it that NO can be made and kept in the laboratory for long periods?arrow_forwardAn experimenter places the following concentrations of gases in a closed container: [NOBr] = 7.13 102 M, [NO] = 1.58 102 M. [Br2] = 1.29 102 M. These gases then react: 2NOBr(g)2NO(g)+Br2(g) At the temperature of the reaction, the equilibrium constant Kc is 3.07 104. Calculate the reaction quotient, Qc, from the initial concentrations and determine whether the concentration of NOBr increases or decreases as the reaction approaches equilibrium. a Qc = 6.33 104; the concentration of NOBr decreases b Qc = 6.33 104; the concentration of NOBr increases c Qc = 1.58 104; the concentration of NOBr increases d Qc = 4.65 104; the concentration of NOBr decreases e Qc = 4.65 104; the concentration of NOBr increasesarrow_forward
- Cyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5H9CH3) but with a different molecular structure. sssss The equilibrium constant has been estimated to be 0.12 at 25 C. If you had originally placed 0.045 mol of cyclohexane in a 2.8-L flask, what would be the concentrations of cyclohexane and methylcyclopentane when equilibrium is established?arrow_forwardBecause calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?arrow_forwardWrite the mathematical expression for the reaction quotient, QC, for each of the following reactions: (a) CH4(g)+CI2CH3CI(g)+HCI(g) (b) N2(g)+O2(g)2NO(g) (c) 2SO2(g)+O2(g)2SO3(g) (d) BaSO3(s)BaO(s)+SO2(g) (e) P4(g)+5O2(g)P4O10(s) (f) Br2(g)2Br(g) (g) CH4(g)+2O2(g)CO2(g)+2H2O(l) (h) CuSO45H2O(s)CuSO4(s)+5H2O(g)arrow_forward
- An equilibrium involving the carbonate and bicarbonate ions exists in natural waters: HCO5_(aq) «=* H+(aq) + COf-(aq) Assuming that the reactions in both directions are elementary' processes: Write rate expressions for the forward and reverse reactions. Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.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 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_forward
- 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_forwardThe equilibrium constant for the dissociation of iodine molecules to iodine atoms I2(g) 2 I(g) is 3.76 103 at 1000 K. Suppose 0.105 mol of I2 is placed in a 12.3-L flask at 1000 K. What are the concentrations of I2 and I when the system comes to equilibrium?arrow_forwardFluorine, F2, dissociates into atoms on heating. 12F2(g)F(g) The value of Kp at 842C is 7.55 102 What is the value of Kc at this temperature?arrow_forward
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