Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![Determine how the addition of extra NO₂ in the previous step will affect the rate constant, Ke
OK, will increase
K, will decrease
OK, will not change
Calculate the equilibrium concentrations of N₂O, and NO₂ after the extra 1.00 mol NO₂ is added to 1.00 L of solution.
[N₂O₁] =
[NO₂] =
mol/L
mol/L](https://content.bartleby.com/qna-images/question/8fa072c0-a0c4-4988-9688-edbe18b8bc58/a4e414ca-66e7-49cd-8af2-a37b3d5f7ab9/xl7lfj6_processed.jpeg)
Transcribed Image Text:Determine how the addition of extra NO₂ in the previous step will affect the rate constant, Ke
OK, will increase
K, will decrease
OK, will not change
Calculate the equilibrium concentrations of N₂O, and NO₂ after the extra 1.00 mol NO₂ is added to 1.00 L of solution.
[N₂O₁] =
[NO₂] =
mol/L
mol/L
Transcribed Image Text:The reaction.
N₂0₁2 NO₂
is allowed to reach equilibrium in a chloroform solution at 25 °C. The equilibrium concentrations are 0.490 mol/L N₂O, and
2.34 mol/L NO₂.
Calculate the equilibrium constant, K., for this reaction.
K₂ =
An additional 1.00 mol NO₂ is added to 1.00 L of the solution and the system is allowed to reach equilibrium again at the
same temperature. Select the direction of the equilibrium shift after the NO, is added.
towards the reactant
towards the product
no change
Determine how the addition of extra NO, in the previous step will affect the rate constant, Ke
Ke will increase
Ke will decrease
Ke will not change
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- produces N20 and oxygen. Calculate the value of the equilibrium constant K. for the reaction 2 N,O4(g) –2 N,0(g) + 3 O2(g) from the following information: N2(g) + ¿O2(g) =N‚O(g) K¸ = 2.7 × 10-18 N,O4(g) =2 NO;(g) K. = 4.6 × 10-3 N2(g) + 2 O2(g) =2 NO2(g) K. = 1.7× 10-17arrow_forwardNitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide. A chemical engineer studying this reaction fills a 125 L tank with 47. mol of nitrogen dioxide gas. When the mixture has come to equilibrium he determines that it contains 22. mol of nitrogen dioxide gas. The engineer then adds another 16. mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits. ||mol x10arrow_forwardSuppose a 500. mL flask is filled with 1.3 mol of Cl₂ and 0.80 mol of HC1. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl (g) The equilibrium constant K for this reaction is 9.14 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M X Ś E A olo 18arrow_forward
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