14. Consider the reaction 2A(g) = B(g) where K- 2.5 at 25 °C. If 0.30 mol A and 0.80 mol B are introduced into a 1.0 L flask at 25 °C, what change in concentrations (if any) will occur in time? a) [A] will decrease and [B] will decrease. b) [A] will increase and [B] will increase. c) [A] will decrease and [B] will increase. d) [A] will increase and [B] will decrease. e) [A] and [B] remain unchanged.

14. Consider the reaction 2A(g) = B(g) where K- 2.5 at 25 °C. If 0.30 mol A and 0.80 mol B are introduced into a 1.0 L flask at 25 °C, what change in concentrations (if any) will occur in time? a) [A] will decrease and [B] will decrease. b) [A] will increase and [B] will increase. c) [A] will decrease and [B] will increase. d) [A] will increase and [B] will decrease. e) [A] and [B] remain unchanged.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.103PAE: 12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat....

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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?
12.42 The following reaction is in equilibrium in lake water: HCO,_(aq) + H+(aq)«=*H,CO,(aq) Predict the change in the reaction quotient, Q, for each disturbance below and use that prediction to explain how the equilibrium is shifted by the stress. NaHCOj is added to the lake. H,CO}is added. NaOH is added.
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.
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For which reactions in Exercise 34 is Kp equal to K?
The following two diagrams represent the composition of an equilibrium mixture for the reaction A2 + B2 2AB at two different temperatures. Based on the diagrams, is the chemical reaction endothermic or exothermic? Explain your answer using Le Chteliers principle. (A atoms are red and B atoms are green in the diagrams.)
For the reaction N2(g)+3H2(g)2NH3(g) show that Kc = Kp(RT)2 Do not use the formula Kp = Kc(RT)5n given in the text. Start from the fact that Pi = [i]RT, where Pi is the partial pressure of substance i and [i] is its molar concentration. Substitute into Kc.
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.
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