The reaction quotient for a system is 68. If the equilibrium constant for the system is 33, what will happen as equilibrium is approached? a. There will be a net gain in both product and reactant. O b. There will be no net gain in either product or reactant. O c. There will be a net gain in product. Od. The equilibrium constant will decrease until it equals the reaction quotient. O e. There will be a net gain in reactant.

The reaction quotient for a system is 68. If the equilibrium constant for the system is 33, what will happen as equilibrium is approached? a. There will be a net gain in both product and reactant. O b. There will be no net gain in either product or reactant. O c. There will be a net gain in product. Od. The equilibrium constant will decrease until it equals the reaction quotient. O e. There will be a net gain in reactant.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 43QAP: . Suppose are action has the equilibrium constant K=1.3108. What does the magnitude of this constant...

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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.
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12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial concentrations are [O3]=1.0106M,[NO]=1.0105M,[NO2]=2.5104M, and [O2]=8.2103M , is the system at equilibrium? If not, in which direction does the reaction proceed? (b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
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?
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