At a particular temperature, Kp=N₂04(9) 2NO₂(g)A flask containing only NO2(g) at an initial pressure of 9.20 atm is allowed to reach equilibrium. Calculate the totalpressure in this flask at equilibrium.Submit Answer0.500 for the reactionIncorrect. Tries 1/99 Previous TriesWith no change in the amount of material in the flask, the volume of the container in question is increased to 7.000 timesthe original. Assuming constant temperature, calculate the (new) total pressure, at equilibrium.Submit Answer Tries 0/99

Answer: According to Dalton's law of partial pressure, total pressure of the system is equal to the…

At a particular temperature, Kp = 0.500 for the reaction N₂04(9) 2NO₂(g) A flask containing only NO2(g) at an initial pressure of 9.20 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium. Submit Answer Incorrect. Tries 1/99 Previous Tries With no change in the amount of material in the flask, the volume of the container in question is increased to 7.000 times the original. Assuming constant temperature, calculate the (new) total pressure, at equilibrium. Submit Answer Tries 0/99

At a particular temperature, Kp = 0.500 for the reaction N₂04(9) 2NO₂(g) A flask containing only NO2(g) at an initial pressure of 9.20 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium. Submit Answer Incorrect. Tries 1/99 Previous Tries With no change in the amount of material in the flask, the volume of the container in question is increased to 7.000 times the original. Assuming constant temperature, calculate the (new) total pressure, at equilibrium. Submit Answer Tries 0/99

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 60QRT

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Similar questions

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Consider the following reactions at some temperature: 2NOCl(g)2NO(g)+Cl2(g)K=1.6105 2NO(g)N2(g)+O2(g)K=11031 For each reaction, assume some quantities of the reactants were placed in separate containers and allowed to come to equilibrium. Describe the relative amounts of reactants and products that would be present at equilibrium. At equilibrium, which is faster, the forward or reverse reaction in each case?
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