3. Chemists always want to find ways to increase the yield of a reaction. equilibrium is the chemist's worst enemy! (At least when a reaction has a small equilibrium constant. Two common ways for a chemist to increase the yield of a reaction are described below. Explain why they increase the yield. It would appear that a. Method 1: Add more of one of the reactants. b. Method 2: Remove one of the products as it is being made.

3. Chemists always want to find ways to increase the yield of a reaction. equilibrium is the chemist's worst enemy! (At least when a reaction has a small equilibrium constant. Two common ways for a chemist to increase the yield of a reaction are described below. Explain why they increase the yield. It would appear that a. Method 1: Add more of one of the reactants. b. Method 2: Remove one of the products as it is being made.

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem SII2RE

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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.)
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
Colorless N2O4 gas decomposes to form red-brown colored NO2 gas. Describe how the concentrations of N2O4 and NO2 would change increase or decrease as equilibrium was established in a sealed container that initially contained only N2O4. What observation would indicate that equilibrium had been established?
. Hydrogen gas, oxygen gas, and water vapor are in equilibrium in a closed container. Hydrogen gas is injected into the container, and the system is allowed to return to equilibrium. Which of the following occurs? Explain your answer. 2H2(g)+O2(g)2H2O(g)a. The concentration of oxygen gas remains constant. b. The value for K increases. c. The concentration of oxygen gas increases. d. The concentration of water vapor increases. e. The value for K decreases.
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. The equilibrium constant for the reaction 2NOCl(g)2NO(g)+Cl2(g)has the value 9.2106at a particular temperature. The system is analyzed at equilibrium, and it is found that the concentrations of NOCl(g) and NO(g) are 0.44 M and 1.5103M. respectively. What is the concentration of Cl2(g) in the equilibrium system under these conditions?
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A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.