G webassign.net B A W Chapter... G N. O LCG a Ⓒ H H The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if K and Q are within 5% of each other.) (a) 2 NH3(9) N₂(g) + 3 H₂(g) [NH3]; = 0.485 M, [N₂]; = 0.160 M, [H₂] = 0.110 M, K = 18 What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. O To the right, i.e. the product-side. O It will not shift. (b) 2 NH3(g) = N₂(g) + 3 H₂(g) What is the reaction quotient? P,(NH3) = 1.90 atm, P,(N₂) = 11.65 atm, P.(H₂) = 11.65 atm, K = 6.6x104 What direction will the reaction shift to? O To the left, i.e. the reactant-side. O To the right, i.e. the product-side. It will not shift. (c) 2 SO 3(g) = 2 SO₂(g) + O₂(g) What is the reaction quotient? [SO3) = 1.65 M, [SO2₂], = 1.65 M, [0₂], = 1.65 M, K = 0.22 What direction will the reaction shift to? To the left, i.e. the reactant-side. O To the right, i.e. the product-side. It will not shift. +

G webassign.net B A W Chapter... G N. O LCG a Ⓒ H H The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if K and Q are within 5% of each other.) (a) 2 NH3(9) N₂(g) + 3 H₂(g) [NH3]; = 0.485 M, [N₂]; = 0.160 M, [H₂] = 0.110 M, K = 18 What is the reaction quotient? What direction will the reaction shift to? O To the left, i.e. the reactant-side. O To the right, i.e. the product-side. O It will not shift. (b) 2 NH3(g) = N₂(g) + 3 H₂(g) What is the reaction quotient? P,(NH3) = 1.90 atm, P,(N₂) = 11.65 atm, P.(H₂) = 11.65 atm, K = 6.6x104 What direction will the reaction shift to? O To the left, i.e. the reactant-side. O To the right, i.e. the product-side. It will not shift. (c) 2 SO 3(g) = 2 SO₂(g) + O₂(g) What is the reaction quotient? [SO3) = 1.65 M, [SO2₂], = 1.65 M, [0₂], = 1.65 M, K = 0.22 What direction will the reaction shift to? To the left, i.e. the reactant-side. O To the right, i.e. the product-side. It will not shift. +

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 following reaction has an equilibrium constant Ke = 1.5. A, + B, =2AB The following diagrams represent reaction mixtures where A is represented by red spheres and B is represented by blue spheres. For each diagram, determine if the reaction mixture is at equilibrium. If it is not at equilibrium, determine the direction in which the reaction will proceed to reach equilibrium.
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Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO2(g)+ H2O(1)-2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 6.6 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 8.7 g H₂O 230.3 g HNO, 10.8 g NO 10.3 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0 I Don't Know Submit 5 ? olo 2024 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
Suppose à 250. mL flask is filled with 1.3 mol of CO, 1.8 mol of H,O and 1.6 mol of H,. This reaction becomes possible: co() +H,0(g) =CO,e)+H,(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H,. You can leave out the M symbol for molarity. CO H,0 Co, H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Roserved Terms of Use Privacy 1 Ace O Type here to search
4. The formation of glucose from water and carbon dioxide is an extremely important reaction for life to exist. Plants perform this reaction through the process of photosynthesis, creating the base of the food chain. The UNBALANCED equation is: H₂O (9) CO2 (g) C6H12O6 (s) + O2 (g) At a particular temperature the equilibrium concentrations were found to be: [H₂0] = 7.90x10-2M, [CO₂] = 0.930M, [0₂] =2.40x10-³M. a. Balance the equation. b. Write an expression for Kc- c. Calculate the value of Kc for the reaction at equilibrium.
Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s)+3 H,0(g)→ Fe,O3(s)+3 H,(g) At a certain temperature, a chemist finds that a 9.2 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound amount ol. Fe 4.85 g Ar H,O 1.44 g Fe,O3 2.98 g H2 2.51 g Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K_ = 0 Ox10 Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility
A mixture of 0.100 mol of SO2 and 0.100 mol of O2 is placed in a reaction container and allowed to react until equilibrium is established. 2 SO2 (g) + O2 (g) -> 2 SO3 At equilibrium, 0.0916 mol of SO3 is present. a. What is the composition of the equilibrium mixture in terms of moles of each substance present? (Hint: Stoichiometry!) b. If the container size is 3.0 L, what is the value of the equilibrium constant?
For the following reaction 2 SO2(g) + O2(g) <-> 2 SO3(g) + heat If the equilibrium situation is stressed by increasing the volume of the container, the reaction will shift toward a No change b Right or products c Left or reactants
Consider the following exothermic reaction system at equilibrium: N2(g) + 3H2(g) ⇒ 2NH3(g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below: Note: Use I for increase, D for decrease, NC for no change Add N2(g) Remove H2(g) Add NH3(9) Add Ne(g) Increase the temperature (constant P) Decrease the volume (constant T) Add a catalyst Submit NH3 N₂ H2