4. Which is an example of a heterogeneous equilibrium system? *a. 2H,(g) + 0,(g) 2H,0(g)b. NO,(g) + NO(g) N,0,(g)c. PCI,(g) PCI,(g) + Cl,(g)d. Cu²+(aq) + 20H (aq) = Cu(OH),(s)e. Fe+(aq) + SCN-(aq) FESCN2+(aq)aO b 5. For the reaction depicted below, which result will occur if the containerexperiences a decrease in volume?*CO(g) + NO,(g)= CO;(g) + NO(g)O There will be no effect on the system.O The reaction will shift to the left.O The reaction will shift to the right.The reaction will heat up.O The reaction will cool down.

"As you have asked multiple Q in a single post, I am gonna help you with the first one. If you need…

4. Which is an example of a heterogeneous equilibrium system? a. 2H,(g) + 0,(g) = 2H,0(g) b. NO,(g) + NO(g)=N,0,(g) c. PCI,(g) = PCI,(g) + Cl,(g) d. Cu2+(aq) + 20H"(aq) = Cu(OH),(s) e. Fe+(aq) + SCN-(ag) = FESCN2+(ag)

4. Which is an example of a heterogeneous equilibrium system? a. 2H,(g) + 0,(g) = 2H,0(g) b. NO,(g) + NO(g)=N,0,(g) c. PCI,(g) = PCI,(g) + Cl,(g) d. Cu2+(aq) + 20H"(aq) = Cu(OH),(s) e. Fe+(aq) + SCN-(ag) = FESCN2+(ag)

Living By Chemistry: First Edition Textbook

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ISBN:9781559539418

Author:Angelica Stacy

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ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

SectionU6.4: How Favorable: Equilibrium Constank K

Problem 1E

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Consider 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?
In 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.
In Section 17.3 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 for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
Because 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?
12.108 A nuclear engineer is considering the effect of discharging waste heat from a power plant into a lake and estimates that this may warm the water locally to 25 °C. One question to be considered is the effect of this temperature change on the uptake of CO2 by the water. The equilibrium constant for the reaction CO2+H2OH2CO3 ; is K=1.7103 at 25 °C. Because bonds form, the reaction is exothermic. (a) Will this reaction progress further toward products at higher temperatures near the water discharge with its warmer water than it would in the cooler lake water? Explain your reasoning. (b) Carbonic acid has a Kaof 2.5104 at 25 °C. What is the equilibrium constant for the CO2+2H2OHCO3+H3O+? (c) What additional factor should the engineer be considering about CO2 gas, probably before considering this reaction chemistry?
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.)
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).]
12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.

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