19eQreqwithdr2req#3EDThe reaction20CForms [Office of t... KB Viewing Your Aca... Have Changes in...Submit Answer$42 NO(g) + Br₂(g) → 2NOBr(g)has Kp = 109 at 25°C. If the equilibrium partial pressure of Br₂ Is 0.0285 atm and the equilibrium partial pressure ofNOBr is 0.0682 atm, calculate the partial pressure of NO at equilibrium.Partial pressure =atm900000 F4RFVShow Hint%5Retry Entire Group 9 more group attempts remainingTFSGCengage Learning Cengage Technical SupportA6B[Review Topics]MacBook AirYH&7NUJ*8➤11FBIM(9Scholarship Ameri... bio 1108 chatK[References]FOO<V.H)OLF10PcommandIA.{+ 11[altSAVAGE X FENTY.....?optionNext#119Save and ExitF121Gdelete

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19 Forms [ Office of t... KB Viewing Your Aca... Have Changes in... The reaction [Review Topics] Submit Answer Scholarship Ameri... bio 1108 chat Retry Entire Group 9 more group attempts remaining [References] 2NO(g) + Br₂ (g) = 2 NOBr(g) has Kp = 109 at 25°C. If the equilibrium partial pressure of Br₂ is 0.0285 atm and the equilibrium partial pressure of NOBr is 0.0682 atm, calculate the partial pressure of NO at equilibrium. Partial pressure = atm SAVAGE X FENTY.....

19 Forms [ Office of t... KB Viewing Your Aca... Have Changes in... The reaction [Review Topics] Submit Answer Scholarship Ameri... bio 1108 chat Retry Entire Group 9 more group attempts remaining [References] 2NO(g) + Br₂ (g) = 2 NOBr(g) has Kp = 109 at 25°C. If the equilibrium partial pressure of Br₂ is 0.0285 atm and the equilibrium partial pressure of NOBr is 0.0682 atm, calculate the partial pressure of NO at equilibrium. Partial pressure = atm SAVAGE X FENTY.....

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 25QAP: Consider the decomposition of ammonium hydrogen sulfide: NH4HS(s)NH3(g)+H2S(g) In a sealed flask at...

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Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the interconversion reaction?
Consider the same reaction as in Question 11. In one experiment 1.0 mole of H2O(g) and 1.0 mole of CO(g) are put into a flask and heated to 350C. In a second experiment 1.0 mole of H2(g) and 1.0 mole of CO2(g) are put into another flask with the same volume as the first. This mixture is also heated to 350C. After equilibrium is reached, will there be any difference in the composition of the mixtures in the two flasks?
The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
The equilibrium constant for the butane iso-butane equilibrium at 25 C is 2.50. Calculate rG at this temperature in units of kJ/mol.
Consider the decomposition of ammonium hydrogen sulfide: NH4HS(s)NH3(g)+H2S(g) In a sealed flask at 25C are 10.0 g of NH4HS, ammonia with a partial pressure of 0.692 atm, and H2S with a partial pressure of 0.0532 atm. When equilibrium is established, it is found that the partial pressure of ammonia has increased by 12.4%. Calculate K for the decomposition of NH4HS at 25C.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure at equilibrium is 40% greater than it was originally, when only I2 was present. What is K for this reaction at that temperature?
For which reactions in Exercise 34 is Kp equal to K?
Consider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial pressure of CO2 at room temperature?
For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of C at 1273 K, will the equilibrium mixture contain (a) mostly CO2? (b) mostly CO? (c) roughly equal amounts of CO2 and CO? (d) only C?
12.42 The following reaction is in equilibrium in lake water: HCO,_(aq) + H+(aq)«=*H,CO,(aq) Predict the change in the reaction quotient, Q, for each disturbance below and use that prediction to explain how the equilibrium is shifted by the stress. NaHCOj is added to the lake. H,CO}is added. NaOH is added.
If wet silver carbonate is dried in a stream of hot air. the air must have a certain concentration level of carbon dioxide to prevent silver carbonate from decomposing by the reaction Ag2CO3(s)Ag2O(s)+CO2(g) H for this reaction is 79.14 kJ/mol in the temperature range of 25 to 125C. Given that the partial pressure of carbon dioxide in equilibrium with pure solid silver carbonate is 6.23 103 torr at 25C, calculate the partial pressure of CO2 necessary to prevent decomposition ofAg2CO3 at 110C. (Hint: Manipulate the equation in Exercise 79.)