Consider the following reaction at equilibrium. Fe;O4(s) + CO(g) = 3 FeO(s) + CO2(g) AH"= -35.9 kJ 1. What effect will removing Fe;O4(s) have on the system? OThe reaction will shift in the direction of products. OThe reaction will shift to the left. ONo change will be observed. OThe equilibrium constant will decrease. OThe equilibrium constant will increase. 2. What effect will increasing the volume of the container have on the system? OThe reaction will shift in the direction of products. OThe reaction will shift in the direction of reactants. ONo change will be observed. OThe equilibrium constant will decrease. OThe equilibrium constant will increase. 3. What effect will increasing the pressure of the reaction mixture have on the system? OThe reaction will shift in the direction of products. OThe reaction will shift in the direction of reactants. ONo change will be observed. OThe equilibrium constant will decrease. OThe equilibrium constant will increase.

Consider the following reaction at equilibrium. Fe;O4(s) + CO(g) = 3 FeO(s) + CO2(g) AH"= -35.9 kJ 1. What effect will removing Fe;O4(s) have on the system? OThe reaction will shift in the direction of products. OThe reaction will shift to the left. ONo change will be observed. OThe equilibrium constant will decrease. OThe equilibrium constant will increase. 2. What effect will increasing the volume of the container have on the system? OThe reaction will shift in the direction of products. OThe reaction will shift in the direction of reactants. ONo change will be observed. OThe equilibrium constant will decrease. OThe equilibrium constant will increase. 3. What effect will increasing the pressure of the reaction mixture have on the system? OThe reaction will shift in the direction of products. OThe reaction will shift in the direction of reactants. ONo change will be observed. OThe equilibrium constant will decrease. OThe equilibrium constant will increase.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The synthesis of CaCO3 uses this chemical reaction. CaO(aq) + CO2(g) ——> CaCO3(s) + 180 kJ Identify three stresses that can be imposed on the equilibrium to maximize the amount of CaCO3 present. Be specific about what, if any, compounds are involved in those stresses.
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Consider the following equilibrium: N2 (g)+3H2(g)2NH3 (g) AG = -34. kJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: OO rise ☐ x10 fall OO Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H2? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm S
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Consider the following system: 4 NH3(g) + 3 O2(g) -> 2 N2(g) + 6 H2O(l) AH = -1530.4 kJ (a) How will the amount of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N,(g)? (3) adding water? (4) expanding the container at constant pressure? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
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