Introductory Chemistry - Access
6th Edition
ISBN: 9781323818893
Author: Tro
Publisher: PEARSON
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Chapter 15, Problem 5SAQ
Consider the reaction between NO and
a. 11
b. 4.3
c. 6.4
d. 0.22
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- 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_forwardConsider the reaction Fe3+(aq)+SCN(aq)FeSCN2+(aq) How will the equilibrium position shift if a. water is added, doubling the volume? b. AgNO3(aq) is added? (AgSCN is insoluble.) c. NaOH(aq) is added? [Fe(OH)3 is insoluble.] d. Fe(NO3)3(aq) is added?arrow_forwardConsider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?arrow_forward
- Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]arrow_forwardWhat is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.arrow_forwardDecomposition of ammonium dichromate is shown in the designated series of photos. In a closed container this process reaches an equilibrium state. Write a balanced chemical equation for the equilibrium reaction. How is the equilibrium affected if more ammonium dichromate is added to the equilibrium system? more water vapor is added? more chromium(III) oxide is added? Decomposition of ammonium dichromate, for Question 4. Decomposition of (NH4)2Cr2O7. Orange, solid (NH4)2Cr2O7 (a) can be ignited by lighting a wick (b), which initiates decomposition (c) forming Cr2O3, the dark green solid in part (d), N2 gas, and water vapor. Energy is transferred to the surroundings by the process.arrow_forward
- Consider the system SO3(g)SO2(g)+12 O2(g)H=98.9kJ (a) Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by 1. adding oxygen gas. 2. compressing the system at constant temperature. 3. adding argon gas. 4. removing SO2(g). 5. decreasing the temperature. (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forwardIn Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.arrow_forwardIn the figure, orange fish are placed in one aquarium and green fish in an adjoining aquarium. The two tanks are separated by a removable partition that is initially closed. (a) Describe what happens in the first few minutes after the partition is opened. (b) What would you expect to see several hours later? (c) How is this system analogous to dynamic chemical equilibrium?arrow_forward
- Write equilibrium expressions for each of the following heterogeneous equilibria. CaCO,(s) ** Ca2+(aq) + COf "(aq) AgCl(s) «=* Ag+(aq) + Cl_(aq) Mg5(PO4)2(s) «=* 3 Mg2+(aq) + 2 PO4J’(aq) Zn(s) + Cu*+(aq) «=* Cu(s) + Zn2+(aq)arrow_forwardConsider the equilibrium process depicted in Fig. 17.6. When does the equilibrium state occur?arrow_forwardConsider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?arrow_forward
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