Consider the following equilibrium:2NO(g) +Cl₂ (g)2NOCI (g) AG° = -41. KJNow suppose a reaction vessel is filled with 2.11 atm of chlorine (C12) and 1.38 atm of nitrosyl chloride (NOC1) at 1123. °C. Answer the following questionsabout this system:riseUnder these conditions, will the pressure of C₁₂ tend to rise or fall?☐ x10fallIs it possible to reverse this tendency by adding NO?In other words, if you said the pressure of C₁₂ will tend to rise, can that bechanged to a tendency to fall by adding NO? Similarly, if you said thepressure of C₁₂ will tend to fall, can that be changed to a tendency to riseby adding NO?If you said the tendency can be reversed in the second question, calculatethe minimum pressure of NO needed to reverse it.Round your answer to 2 significant digits.yesnoatmG

the pressure of Cl2 will fall in first step and rise in second step when pressure of NOCl will be…

Answered: Consider the following equilibrium:…

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 a 250. mL flask is filled with 1.9 mol of Br,, 1.8 mol of BrOCl and 1.6 mol of BrCl. The following reaction becomes possible: Br, (g) + OC1, (g) = BIOC1(g) + BrC1(g) The equilibrium constant K for this reaction is 4.15 at the temperature of the flask. Calculate the equilibrium molarity of Br,. Round your answer to two decimal places. 0.53 M ?
1. Consider the following hypothetical reaction at equilibrium: 2A (g) + B (g) = 2C (g) At 400 K, the value of the equilibrium constant K. = 4.15 x 10* Based on this K, does the equilibrium favor the reactants or the products? Why?
Consider the general reaction 2A(g) + B(s) = C(g) +3D(g) AH = +115 kJ which has already come to equilibrium The position of the equilibrium was shifted by adding additional B(s) to the system. Choose the correct effect on equilibrium (it will shift to the right, will shift to the left, or it will not be affected). O It will shift to the right. O It will shift to the left. O It will not be affected Consider the general reaction 2A(9) + B(s) C(g) + 3D(g) AH = +115 kJ which has already come to equilibrium. The position of the equilibrium was shifted by removing C(g) from the system as it forms. Choose the correct effect on equilibrium (it will shift to the right, will shift to the left, or it will not be affected). O It will shift to the right. O It will shift to the left. O It will not be affected.
6. A quantity of liquid methanol, CH3OH, is introduced into a rigid 3.00-L vessel, the vessel is sealed, and the temperature is raised to 500K. At this temperature, the methanol vaporizes and decomposes according to the reaction CH3OH(g) → CO(g) + 2 H2(g), Ke= 6.90×10-². If the concentration of H₂ in the equilibrium mixture is 0.426M, what mass of methanol was initially introduced into the vessel?
Help with the following question. Please round the answer to 2 decimal places
Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. The equilibrium will not shift The equilibrium will shift toward product but Keq will not change The equilibrium will shift toward reactant but Keq will not change The equilibrium will shift toward product but Keq will will increase The equilibrium will shift toward reactant but Keq will decrease(b) The reaction mixture is cooled. (c) The volume of the reaction vessel is reduced by 50%.
Write equilibrium expressions for: N₂(g) + 3H₂(g) 2NH₂(g) 3 the reaction as written • the reverse reaction the reaction as written with all coefficients in the equation halved
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.
Steam reforming of methane ( CH, ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the starting point for many important industrial chemical syntheses. An industrial chemist studying this reaction fills a 2.0 L flask with 1.9 atm of methane gas and 2.1 atm of water vapor, and when the mixture has come to equilibrium measures the partial pressure of hydrogen gas to be 4.6 atm. Calculate the pressure equilibrium constant for the steam reforming of methane at the final temperature of the mixture. Round your answer to 2 significant digits. K, = 0
Suppose a 250. mL flask is filled with 1.2 mol of Br,, 1.4 mol of OCl, and 1.1 mol of BrCl. The following reaction becomes possible: Br, (g) +OCl, (g) - BrOC1 (g) +BrC1(g) The equilibrium constant K for this reaction is 0.483 at the temperature of the flask. Calculate the equilibrium molarity of OCl,. Round your answer to two decimal places. OM
Consider the following reaction:COCl2(g) CO(g) + Cl2(g) If 1.64×10-3 moles of COCl2(g), 0.398 moles of CO, and 0.360 moles of Cl2 are at equilibrium in a 18.2 L container at 843 K, the value of the equilibrium constant, Kc, is .
Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4(9) +20 2(g) =CO2(g) + 2H 20(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is reduced? O a. The equilibrium position is shifted to the left and the value for K increases. O b. The equilibrium position is shifted to the right and the value for K increases. O c. The equilibrium position is shifted to the right and the value for K decreases. O d. The equilibrium position is shifted but the value for K stays constant. Oe. The equilibrium position is shifted to the left and the value for K decreases.

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