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2. Determine Ke for the reaction (Answer: 9.7x10-16): 2 N2(g) + 1/2O2(g) + Brz(g) $ NOBr...
14.39. The K value for the reaction 2 NOBr(g) – 2 NO(g) + Brz(8) is 3.0...
14.39. The K value for the reaction 2 NOBr(g) – 2 NO(g) + Brz(8) is 3.0 X 10-4 at 298 K. What is the value of Kc at 298 K for the following reaction? NOBr(g) – NO(g) + 2 Br2(g)
The equilibrium constant for the reaction 2 NO(g) + Br2 = 2 NOBr(9) is Ke = 2.4 x 10-2 at certain temperature. Calc...
The equilibrium constant for the reaction 2 NO(g) + Br2 = 2 NOBr(9) is Ke = 2.4 x 10-2 at certain temperature. Calculate K for 2 NOBr(9) = 2 NO(g) + Brz (9) Express your answer using two significant figures. V AEC O ? K- Submit Request Answer Part C Complete previous part(s)
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related...
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
. Determine the value of the equilibrium constant for the reaction N2 (g) + 2O2 (g)...
. Determine the value of the equilibrium constant for the reaction N2 (g) + 2O2 (g) ↔ N2O4 (g) from the following equations. ½ N2 (g) + ½ O2 (g) ↔ NO (g) KC = 6.9 x 10-16 2NO2 (g) ↔ 2NO (g) + O2 (g) KC = 4.5 x 10-13 2NO2 (g) ↔ N2O4 (g) KC = 6.7
The equilibrium constant for the reaction 2 NO(g) + Br2 = 2 NOBr(9) is Ke =...
The equilibrium constant for the reaction 2 NO(g) + Br2 = 2 NOBr(9) is Ke = 2.2 x 10" at certain temperature. K = 45 Previous Answers Correct Correct answer is shown. Your answer 45.45 was either rounded differes significant figures than required for this part. Part 6 Calculate K. for NOBr(g) - NO(g) + Bra(g). Express your answer using two significant figures. A = 0 ?
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...
z 5. Consider the following equilibria in aqueous solution at room temperature: 2NO(g) = N2(g) +...
z 5. Consider the following equilibria in aqueous solution at room temperature: 2NO(g) = N2(g) + O2 (8) K= 1.0 x 10" N2(g) + O2 (6) + Br2 (8) = 2NOBrg) K = 2.0 x 10" Find the numerical value of K for the reaction 2 NOBr (g) = 2 NO (g) + Br2 (g) a) 2.0 x 103 b) 5.0 x 1056 C) 1.0 x 1030 d) 5.0 x 10-4
Consider the reaction: 2 NO(g) + Br2(g) ↔ 2 NOBr(g) Kp = 28.4 atm-1 at 298 K...
Consider the reaction: 2 NO(g) + Br2(g) ↔ 2 NOBr(g) Kp = 28.4 atm-1 at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 173 Torr and that of Br2 is 142 Torr. What is the partial pressure (in Torr) of NOBr in this mixture? PNOBr = ___ Torr
27. Consider the following chemical reaction: N2(g) + 2O2(g) ----> 2NO2(g) decreasing the pressure of reaction...
27. Consider the following chemical reaction: N2(g) + 2O2(g) ----> 2NO2(g) decreasing the pressure of reaction mixture will decrease amounts of O2(g) have no effect on the reaction increase amounts of N2(g) increase amounts of NO2(g) 26. Consider the following chemical reaction: CO(g) + Cl2(8) ----------> COCl2(g) At the beginning 0.400 M CO(g) is mixed with 0.0500 M C12(8). At equilibrium, 0.0100 M of the product is produced. Calculate the equilibrium constant. K-0.641 K - 1.99x 10exp-3 K-8.81 OK -...
Nitrosyl bromide decomposes by the reaction 2 NOBO(g) + 2NO(9) + Brz(9). Show that the following...
Nitrosyl bromide decomposes by the reaction 2 NOBO(g) + 2NO(9) + Brz(9). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. Students may do this by plotting the data three different ways. For each plot, time goes on the x-axis. A zero-order reaction is linear when [NOBr] on the y-axis. A first-order reaction is linear when In[NOBr) is on the y-axis. A second-order reaction is linear when 1/[NOBr) is...
14.39. The K value for the reaction 2 NOBr(g) – 2 NO(g) + Brz(8) is 3.0 X 10-4 at 298 K. What is the value of Kc at 298 K for the following reaction? NOBr(g) – NO(g) + 2 Br2(g)
The equilibrium constant for the reaction 2 NO(g) + Br2 = 2 NOBr(9) is Ke = 2.4 x 10-2 at certain temperature. Calculate K for 2 NOBr(9) = 2 NO(g) + Brz (9) Express your answer using two significant figures. V AEC O ? K- Submit Request Answer Part C Complete previous part(s)
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...
The equilibrium constant for the reaction 2 NO(g) + Br2 = 2 NOBr(9) is Ke = 2.2 x 10" at certain temperature. K = 45 Previous Answers Correct Correct answer is shown. Your answer 45.45 was either rounded differes significant figures than required for this part. Part 6 Calculate K. for NOBr(g) - NO(g) + Bra(g). Express your answer using two significant figures. A = 0 ?
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...
z 5. Consider the following equilibria in aqueous solution at room temperature: 2NO(g) = N2(g) + O2 (8) K= 1.0 x 10" N2(g) + O2 (6) + Br2 (8) = 2NOBrg) K = 2.0 x 10" Find the numerical value of K for the reaction 2 NOBr (g) = 2 NO (g) + Br2 (g) a) 2.0 x 103 b) 5.0 x 1056 C) 1.0 x 1030 d) 5.0 x 10-4
27. Consider the following chemical reaction: N2(g) + 2O2(g) ----> 2NO2(g) decreasing the pressure of reaction mixture will decrease amounts of O2(g) have no effect on the reaction increase amounts of N2(g) increase amounts of NO2(g) 26. Consider the following chemical reaction: CO(g) + Cl2(8) ----------> COCl2(g) At the beginning 0.400 M CO(g) is mixed with 0.0500 M C12(8). At equilibrium, 0.0100 M of the product is produced. Calculate the equilibrium constant. K-0.641 K - 1.99x 10exp-3 K-8.81 OK -...
Nitrosyl bromide decomposes by the reaction 2 NOBO(g) + 2NO(9) + Brz(9). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. Students may do this by plotting the data three different ways. For each plot, time goes on the x-axis. A zero-order reaction is linear when [NOBr] on the y-axis. A first-order reaction is linear when In[NOBr) is on the y-axis. A second-order reaction is linear when 1/[NOBr) is...
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