The following reaction components are at equilibrium, and the reaction is exothermic in the direction written below. Which change will shift the equilibrium in a direction that will result in increasing concentration of SO2 in the container? 2 SO2(3) + O2(g) =2 SO3(g) raising the temperature decreasing the temperature Removing SO3 from the reaction mixture O Adding O2 to the reaction mixture

The following reaction components are at equilibrium, and the reaction is exothermic in the direction written below. Which change will shift the equilibrium in a direction that will result in increasing concentration of SO2 in the container? 2 SO2(3) + O2(g) =2 SO3(g) raising the temperature decreasing the temperature Removing SO3 from the reaction mixture O Adding O2 to the reaction mixture

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 oxidation of ammonia is a reversible exothermic reaction at equilibrium that proceeds as follows: 4 NH3 (g) + 5 O2 (g) ⇋ 4 NO (g) + 6 H2O (g) If the concentration of NO is added what happens to the concentration of H2O?
choose ONE of each of the red selections. for example you choose between endothermic or exothermic and fill out the other options to make the statement true
The oxidation of ammonia is a reversible exothermic reaction at equilibrium that proceeds as follows: 4 NH3 (g) + 5 O2 (g) ⇋ 4 NO (g) + 6 H2O (g) If the concentration of NH3 is increased what happens to the concentration of NO?
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For this reaction, the equilibrium constant, Kea, is 6.1 x 10-4 SO3 (g) - O2 (g) + 2SO3 (g) Select the most accurate statement. O the equilibrium favors reactants O the rate of the forwards reaction is very fastfast O at equilibrium, the reaction mixture will contain a lot of both reactants and products O the rate of the forwards reaction is very slow O the equilibrium favors products
. Consider the equilibrium 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H₂O(g). Predict the effect on the equilibrium concentration by the addition of N₂. A The equilibrium will shift to produce more nitrogen. B The equilibrium will shift to produce more reactants. C The equilibrium will shift to produce more products. D The reaction is already at equilibrium. E None of the above Given: 2P(g) + 3Cl2(g) → 2PC13(g) K Calculate the equilibrium constant for the following reaction. P(g) + 3/2Cl2(g) → PCI(g) AK BK¹ C 2K D 0.5K EK¹/2
(a) At 2000°C, the equilibrium constant for the reaction: N2(g) + O2(g) ó 2 NO(g) is 4.1 x 10-4 If the initial concentration are [N2] = 0.2 M and [O2] = 0.1 M, how much of each of the components will be present at equilibrium?
Consider the following reaction and its equilibrium constant: 12 (g) + Br2 (g) ÷ 2 IBr (g) Kc = 1.1 × 102 A reaction mixture contains 0.41 M I2, 0.27 M Br2 and 2.2 M IBr. Which of the following statements is TRUE concerning this system? O The equilibrium constant needs to increase. The reaction needs to shift in the direction of the reactants to reach equilibrium. O The system is at equilibrium. O The reaction needs to shift in the direction of the products to reach equilibrium.
For the following reaction at equilibrium, which of the changes below would cause the equilibrium to shift to the right and form more products? 2 NOBR(g) + 2 NO(g) + Br2(g) A H°n = 30 kJ/mol Increase the temperature Increase the container volume Remove some NO Add some NOBr
Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 104M. N2(g) + 3H2(g) = 2NH3(g) 3. BI U T O Word(s) 4. If the concentration of the reactant H2 was decreased from 1.0 x 10-² M to 2.7 x 10-4 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. BI U T O Word(s)
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