Question 13 What is the equilibrium constant expression for the following reaction?2NO2(g)N₂04(9)O a.[NO₂]K₁- [N₂0₂]Ob.K. =[N₂04][NO₂]O C. Kc = [NO₂]²[NO₂]2[N₂O.][N₂O.][NO₂]

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What is the equilibrium constant expression for the following reaction? 2NO2(g) · N₂O4(9) O a. K.- = O b. = e. [NO₂] [N₂04] [N₂04] [NO₂] Oc. Kc = [NO₂1² [NO₂]² K₁- [N₂0.] [N₂O₁] [NO₂]2 P

What is the equilibrium constant expression for the following reaction? 2NO2(g) · N₂O4(9) O a. K.- = O b. = e. [NO₂] [N₂04] [N₂04] [NO₂] Oc. Kc = [NO₂1² [NO₂]² K₁- [N₂0.] [N₂O₁] [NO₂]2 P

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section15.6: Disturbing A Chemical Equilibrium

Problem 3RC

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1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
For the reaction NH3(g)+H2S(g)NH4HS(s) K = 400. at 35.0C. If 2.00 moles each of NH3, H2S, and NH4HS are placed in a 5.00-L vessel, what mass of NH4HS will be present at equilibrium? What is the pressure of H2S at equilibrium?
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