(a)
Interpretation:
Whether the system reaches equilibrium or not has to be determined.
Concept Introduction:
The condition of equilibrium is a state of balance of processes that runs in opposite directions. At equilibrium, the formation of product from reactant balanced the formation of reactant from product. Also, the change in concentration of reaction and product seems to be negligible at equilibrium state.
The general equilibrium reaction is as follows:
Here,
The relation of equilibrium constant
Here,
The formula to calculate the value of
The value of
A reaction quotient
The general equilibrium reaction is as follows:
Here,
The expression of the equilibrium constant for the above reaction is as follows:
Here,
The concentration of reactants and products changes in order to bring reaction quotient and equilibrium constant closer. Therefore, the direction of reaction can be predicted as follows:
(1) If
(2) If
(3) If
(a)
Answer to Problem 14.94QE
The system is not in equilibrium.
Explanation of Solution
The given reaction is as follows:
Substitute 1 for the total number of moles of gas on product side and 2 for the total number of moles of gas on reactant side in equation (2).
Rearrange equation (1) to calculate
The formula to convert degree Celsius to Kelvin is as follows:
Substitute
Substitute
The concentration of
The concentration of
The concentration of
The formula to calculate
Substitute
Since
(b)
Interpretation:
The expected mass of
Concept Introduction:
The expression of the equilibrium constant for the above reaction is as follows:
Here,
(b)
Answer to Problem 14.94QE
The expected mass of
Explanation of Solution
The given reaction is as follows:
The ICE table for the above reaction is as follows:
The expression to calculate
Substitute
Rearrange the above equation as follows:
Solve the quadratic equation for
Or,
But
Therefore the concentration of
The mass of
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Chapter 14 Solutions
Chemistry: Principles and Practice
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- Write equilibrium-constant expressions Kp for each of the following reactions: a H2(g)+Br2(g)2HBr(g) b CS2(g)+4H2(g)CH4(g)+2H2S(g) c 4HCl(g)+O2(g)2H2O(g)+2Cl2(g) d CO(g)+2H2(g)CH3OH(g)arrow_forwardThe equilibrium constant Kc for the synthesis of methanol, CH3OH. CO(g)+2H2(g)CH3OH(g) is 4.3 at 250C and 1.8 at 275C. Is this reaction endothermic or exothermic?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
- 12.103 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_forwardThe equilibrium constant Kc, for the reaction 2 NOCI(g) 2 NO(g) + Cl2(g) is 3.9 103 at 300 C. A mixture contains the gases at the following concentrations: [NOCl] = 5.0 103 mol/L, [NO] = 2.5 103 mol/L, and [Cl2] = 2.0 103 mol/L. Is the reaction at equilibrium at 300 C? If not, in which direction does the reaction proceed to come to equilibrium?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
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