30) For the following reaction, the equilibrium concentration of No2 is 0.38 M and equilibrium concentration...
17) For the reaction N204 (aq) NO2 (aq) Kc-0.360 at 100 "C At 100 °C, the initial conentration of NO2 is 0.0500 M, and there is no N204. Find the concentration of NO2 unds once the system reaches equilibrium at this temperature. D) 0.00457 M E) 0.0380 M A) 0.0022 M B) 0.0361 M C) 0.0408 M 25) For the reaction: A (aq) B (aq),Kc 6.210 The initial, non-equilibrium, concentration of A is 1.6 M, and no B is present....
47. For the following reaction: NO2 Concentration N204 Equilibrium achieved 0 Time (a) Which of the following statements is true? A) At equilibrium, the concentration of reactants and products must change with time. B) At equilibrium, a particular ratio of concentration terms does not equal a constant. C) For equilibrium to occur, neither reactants nor products can escape from the system. D) This reaction does go to stoichiometric completion.
7. The gas phase dimerization reaction 2N02= N204 has an equilibrium constant of K = 4.72 at 373 K (when all concentrations are measured in M units). a) What is AGⓇ for this reaction? b) At what reactant and product concentrations is the reaction free energy equal to AGº? c) Use the quadratic equation to obtain an expression for NO2 as a function of the total nitrogen concentration NT = NO2 + 2 N204), and plot both NO2 and (N204]...
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Find the equilibrium concentration expression for the following reaction N204g) - 2NO2(g) a. Kc = [N20412 [N04] b. Kc= [NO2)? [N204] Kc= [NO2] [N204) d. Kc = [NO21-2 [N204)
5. The equilibrium constant K for the dissociation of N204(g) to NO2(g) is 1700 at 500 K. If AH is 56.8 kJ/mol for this reaction, what will be the value of K at 300 K? (a) 132x106 (b) 1.11 x 104 (c) 0.188 (d) 15.5 (e) .54 x 107
5. The equilibrium constant K for the dissociation of N204(g) to NO2(g) is 1700 at 500 K. If AH is 56.8 kJ/mol for this reaction, what will be the value of...
2. The following species exist in equilibrium: 2 NO2(g) N204 (g). 0.625 moles of N204 were introduced into a 5.00 L vessel and was allowed to decompose until equilibrium was reached. At equilibrium, the concentration of N204 was 0.0750 M Calculate the Kc for the reaction.
22. The initial pressure of N204 = 0.14 atm and the initial pressure of NO2 = 0.55 atm. If the Kp for the reaction is 4.32, what is the equilibrium pressure of the NO2 gas? N2O4 (g) 2 NO2 (g) a) 0.0949 atm b) 0.0451 atm c) 0.658 atm d) 0.640 atm e) 0.731 atm x = - -b + vb2 - 4ac 2a
The equilibrium constant, K, for the reaction N204(g) = 2N02 (8) is 4.8 x 10-3 If the equilibrium mixture contains NO2 = 0.051 M , what is the molar concentration of N, 04? Express the concentration to two significant figures and include the appropriate units. TH A Roa? N, 04] = Value
Dinitrogen tetroxide decomposes to produce nitrogen dioxide: N204 (9) - 2 NO2 (g) Calculate the equilibrium constant for the reaction given the equilibrium concentrations at 100°C: [N204] = 0.800 M and [NO2] = 0.400 M A. 5.00 OB.0.200 OC. 0.500 OD.2.00
When heated, colorless dinitrogen tetraoxide, N204(8), decomposes into red-brown nitrogen dioxide, NO2(g), according to the following reaction: N204(g) 42 NO2 (g) Suppose that 2.00 mol of N204(8) was placed into an empty 5.00-L flask and heated to 407 K. When equilibrium was attained, the concentration of red-brown NO2(g) was found to be 0.525 M. Calculate the equilibrium constant, K., for this reaction at 407 K. 0.500 O 0.525 2.00 0.263 3.80