Consider the equilibrium reaction below: N₂O5(s) + O2(g) = N₂O4(g) + O3(g) Create an equilibrium constant, K, expression for the above reaction using the drag and drop tools: (Reminder:solutes (aq) or gases (g) appear; solvents (1) or solids (s) do not.) K= [N₂O4][03] [N₂O4]+[03] [N₂O5][0₂] [N₂05]+[0₂] [0₂] [N₂O5]

Consider the equilibrium reaction below: N₂O5(s) + O2(g) = N₂O4(g) + O3(g) Create an equilibrium constant, K, expression for the above reaction using the drag and drop tools: (Reminder:solutes (aq) or gases (g) appear; solvents (1) or solids (s) do not.) K= [N₂O4][03] [N₂O4]+[03] [N₂O5][0₂] [N₂05]+[0₂] [0₂] [N₂O5]

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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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. Consider the two reactions given below. Reaction REACTION A REACTION B Equation • 20,(g) = 3 0,(g) N,(g) + 0,(g) =2 NO(g) Picture 1/ K value K = 3.5x10-89 (very small) K = 1.0x1025 (very large) [C Write the K = equilibrium K = [A]1 or <1? Which is mnore common in the reaction mixture: reactants or products?
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 2 CH4(g) = C,H2(g) + 3 H2(g) K, = 1. × 10 He fills a reaction vessel at this temperature with 10. atm of methane gas. Use this data to answer the guestions in the table below. Can you predict the equilibrium pressure of C,H,, using only the О yes tools available to you within ALEKS? O no If you said yes, then enter the equilibrium pressure of C,H, at atm right. Round your answer to 1 significant digit.
The equilibrium system shown below was analyzed and the concentrations of H2(g), I2(g) and HI(g), were found, in mol/L, to be 4.2, 3.8, 1.6 respectively. The equilibrium constant must be? H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
Identify the proper form of the equilibrium-constant expression for the equation N2 (g) + O2 (g) = 2NO(g) • View Available Hint(s) [NO] Ο Κ: [N2][O2] [NO]? O K: [N2][O2] 12 [N2][O2] O K = [NO]? 2[NO] Ο Κ- [N2][O2]
Suppose a 250. mL flask is filled with 1.2 mol of OCl,, 1.9 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br,(g) +OCl,(g) BROCI(g) +BrC1(g) The equilibrium constant K for this reaction is 1.94 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places.
The chemical equation for an equilibrium is described below. kJ mol CaO (s) + CO2(g) = CaCO3(s) AH° Predict how the following changes would shift the equilibria. Be sure to start by writing the equilibrium (K) equation. =-176-
Suppose a 500. mlL flask is filled with 2.0 mol of NO,, 0.30 mol of CO and 1.3 mol of NO. The following reaction becomes possible: NO, (2) + CO(u) - NO()+co,@) The equilibrium constant K for this reaction is 6.41 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
Suppose a 250. ml. flask is filled with 0.20 mol of NO,, 1.6 mol of CO and 0.90 mol of NO. The following reaction becomes possible: NO,()+co(2) NO()+co,@) The equilibrium constant K for this reaction is 0.402 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places.
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Q3. a) Consider this equilibrium system: CO(g) + 2 H2(g) ► CH;OH(1) Find the Ke expression (write the equation). b) Consider this equilibrium system: 2SO,(g) + O2(g) – 2S0;(g) ΔΗ<0. Explain how we could be able to increase the yield of SO:(g)? (remember which factors will influence the reaction yield).
O KINETICS AND EQUILIBRIUM Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.9 mol of NO,, 0.10 mol of N0 and 1.7 mol of CO,. The following reaction becomes possible: 2' NO,(g)+CO(g) -NO(g)+CO,(g The equilibrium constant K for this reaction is 4.70 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M TRADIS Explanation Check 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy | Acces NOV 242 PAGES étv 4 MacBook Air II