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10. Consider the equilibrium reaction: N204(g) + 2NO2(g) Which of the following correctly describes the relationship...
10. The equilibrium constant for the reaction N204(8) = 2NO2(g) at 25 °C is 5.88 x...
10. The equilibrium constant for the reaction N204(8) = 2NO2(g) at 25 °C is 5.88 x 10-3. Suppose 15.6 g of N204(g) is placed in a 5.000-L flask at 25 °C. Calculate the following: (a) The moles of NO2(g) present at equilibrium (b) The percent dissociation of the original N,O4(g).
CHEM 106 Chemical Equilibrium, Acids and Bases 1. Which expression correctly describes the equilibrium constant for...
CHEM 106 Chemical Equilibrium, Acids and Bases 1. Which expression correctly describes the equilibrium constant for the following reaction? 4NH,(g)+ SO,(g) 4NO(g)+ 6H2O) K. LNO"CHO B) K-(4INOj+ 6HO1) (4NH,]+ S10))CAT6 ) K-(INOl,0])INH,O,l) D K-(INOjHO)/(IINH iol) E) K-(NHJTO) /INO)THO ANS: D 2. Determine the equilibrium constant for the system N;Oa 2NO; at 25 C. The concentrations are shown here: [N;O ]-2.32 x 10 A) 0.608 B) 1.65 C) 1.17 x 10 D) 0.369 E) 8.57 x 10 M, [NO 2]-1.41 x...
16. Consider the reaction: 2NO2(g) = N204(g) 4,Hº = -58.04 kJ/mol. Which of the following prediction...
16. Consider the reaction: 2NO2(g) = N204(g) 4,Hº = -58.04 kJ/mol. Which of the following prediction about the color change of system is CORRECT knowing that NO2 is brown and N204 is colorless (assuming all other side reactions can be neglected)? A. If the system at equilibrium is heated up, the color of the gas fades away. B. When the total pressure of the system at equilibrium is increased, the color of the gas deepens. C. If a colorless inert...
5. (10 pts) A 1.00 L reaction vessel is filled with N204 (g) at a pressure...
5. (10 pts) A 1.00 L reaction vessel is filled with N204 (g) at a pressure of 0.154 atm. The gas is then allowed to decompose by the following equilibrium process N204(g) ^ 2NO2(g) a) At equilibrium, the total pressure in the container is 0.212 atm. What is the equilibriunm pressure of NO2 (g)? b) What is the Kp (numerical value) for the above equilibrium process?
2. For the isomerization reaction, N204(g) + 2NO2(g), the degree of dissociation (a) is 0.201 at...
2. For the isomerization reaction, N204(g) + 2NO2(g), the degree of dissociation (a) is 0.201 at equilibrium (25°C and 1 bar). (NOTE: DO NOT simply look up the thermodynamic table for this question. You MUST compute all the quantities using known formula.) (a) Calculate A,G,A,Gº and K at equilibrium. (b) If the equilibrium constant at 100°C is 17.46, is this reaction exothermic or endothermic? (c) Calculate the standard reaction entropy, A. Sº, of this reaction.
The equilibrium constant (K) is 0.13 at a particular temperature for the reaction: N204(g) 2NO2(9) Given...
The equilibrium constant (K) is 0.13 at a particular temperature for the reaction: N204(g) 2NO2(9) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? PNo2-0.107 atm, PN20-0.146 atm Po2 -0.206 atm, Po, 0.136 atm PNo2-0.093 atm,P00.066...
Question text Calculate the equilibrium constants, KpKp and KcKc for the equilibrium reaction N2O4(g)⇄2NO2(g)N2O4(g)⇄2NO2(g) at 298...
Question text Calculate the equilibrium constants, KpKp and KcKc for the equilibrium reaction N2O4(g)⇄2NO2(g)N2O4(g)⇄2NO2(g) at 298 K. N2O4(g)N2O4(g) NO2(g)NO2(g) S0S0 (J/K/mol) 304.29 240.06 ΔfH0ΔfH0 (kJ/mol) 9.16 33.18 Select one or more: A. Kp=9.23Kp=9.23 , Kc=12.3Kc=12.3 B. Kp=0.563Kp=0.563 , Kc=0.33Kc=0.33 C. Kp=0.144Kp=0.144 , Kc=0.0058Kc=0.0058 D. Kp=0.355Kp=0.355 , Kc=1.23
Consider the decomposition of N204(g) into NO2(g). N204(g) = 2 NO2(g) kp = 47.9 at 400...
Consider the decomposition of N204(g) into NO2(g). N204(g) = 2 NO2(g) kp = 47.9 at 400 K Suppose that 1.00 atm of N204 decomposes and reaches equilibrium at 400 K. Determine the partial pressure of NO2 at equilibrium. 1.96 atm 0.922 atm 1.92 atm 0.960 atm 0.979 atm
Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give...
Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give the following information (298.15 K) NO (g) +1/2Br2(g) NOBr(g) Ke 4.5 2 NO (g)N2(g) 02(g) Ke 3.0 x 102 5. For the BrCl decomposition reaction 2BrCl(g) Br2(g Cl2(g) Initially, the vessel is charged at 500 K with BrCl at a partial pressure of 0.500 atm. At equilibrium, the partial pressure of BrC is 0.040 atm. Calculate Kp value at 500K
Consider the...
help pls Find the equilibrium concentration expression for the following reaction N204g) - 2NO2(g) a. Kc...
help pls
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)
10. The equilibrium constant for the reaction N204(8) = 2NO2(g) at 25 °C is 5.88 x 10-3. Suppose 15.6 g of N204(g) is placed in a 5.000-L flask at 25 °C. Calculate the following: (a) The moles of NO2(g) present at equilibrium (b) The percent dissociation of the original N,O4(g).
CHEM 106 Chemical Equilibrium, Acids and Bases 1. Which expression correctly describes the equilibrium constant for the following reaction? 4NH,(g)+ SO,(g) 4NO(g)+ 6H2O) K. LNO"CHO B) K-(4INOj+ 6HO1) (4NH,]+ S10))CAT6 ) K-(INOl,0])INH,O,l) D K-(INOjHO)/(IINH iol) E) K-(NHJTO) /INO)THO ANS: D 2. Determine the equilibrium constant for the system N;Oa 2NO; at 25 C. The concentrations are shown here: [N;O ]-2.32 x 10 A) 0.608 B) 1.65 C) 1.17 x 10 D) 0.369 E) 8.57 x 10 M, [NO 2]-1.41 x...
16. Consider the reaction: 2NO2(g) = N204(g) 4,Hº = -58.04 kJ/mol. Which of the following prediction about the color change of system is CORRECT knowing that NO2 is brown and N204 is colorless (assuming all other side reactions can be neglected)? A. If the system at equilibrium is heated up, the color of the gas fades away. B. When the total pressure of the system at equilibrium is increased, the color of the gas deepens. C. If a colorless inert...
5. (10 pts) A 1.00 L reaction vessel is filled with N204 (g) at a pressure of 0.154 atm. The gas is then allowed to decompose by the following equilibrium process N204(g) ^ 2NO2(g) a) At equilibrium, the total pressure in the container is 0.212 atm. What is the equilibriunm pressure of NO2 (g)? b) What is the Kp (numerical value) for the above equilibrium process?
2. For the isomerization reaction, N204(g) + 2NO2(g), the degree of dissociation (a) is 0.201 at equilibrium (25°C and 1 bar). (NOTE: DO NOT simply look up the thermodynamic table for this question. You MUST compute all the quantities using known formula.) (a) Calculate A,G,A,Gº and K at equilibrium. (b) If the equilibrium constant at 100°C is 17.46, is this reaction exothermic or endothermic? (c) Calculate the standard reaction entropy, A. Sº, of this reaction.
The equilibrium constant (K) is 0.13 at a particular temperature for the reaction: N204(g) 2NO2(9) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? PNo2-0.107 atm, PN20-0.146 atm Po2 -0.206 atm, Po, 0.136 atm PNo2-0.093 atm,P00.066...
Consider the decomposition of N204(g) into NO2(g). N204(g) = 2 NO2(g) kp = 47.9 at 400 K Suppose that 1.00 atm of N204 decomposes and reaches equilibrium at 400 K. Determine the partial pressure of NO2 at equilibrium. 1.96 atm 0.922 atm 1.92 atm 0.960 atm 0.979 atm
Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give the following information (298.15 K) NO (g) +1/2Br2(g) NOBr(g) Ke 4.5 2 NO (g)N2(g) 02(g) Ke 3.0 x 102 5. For the BrCl decomposition reaction 2BrCl(g) Br2(g Cl2(g) Initially, the vessel is charged at 500 K with BrCl at a partial pressure of 0.500 atm. At equilibrium, the partial pressure of BrC is 0.040 atm. Calculate Kp value at 500K
Consider the...
help pls
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)
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