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![Answer: Na (2) + 02 (2) 2 NO (2) The Equilibrium concentration [N2] = 0.24219 [02] = 0.228M (NOJ = 0.061 M At Equilibrium, Kc](http://img.homeworklib.com/questions/285bc270-8cdf-11eb-9ff4-3d4908fcc1b8.png?x-oss-process=image/resize,w_560)
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Use the information in this question to answer questions 29-30. For the equilibrium: N2(g) + O2(g)...
For the Equilibrium System N2 (g) + O2 (g) === 2 NO (g) 1.) Write a...
For the Equilibrium System N2 (g) + O2 (g) === 2 NO (g) 1.) Write a Kc and a Kp expression. 2.) If Kc = 1.50 x 10-2 at 653oC, Calculate and report the equilibrium concentrations of all of the reactants and all of the products at 653oC, if the initial concentrations were [N2]0 = 0.0100 M [O2]0 = 0.0200 M [NO]0 = 0.00300 M 3.) Calculate Kp for this equilibrium system at 653oC using the equation Kp = Kc(RT)∆n....
The reaction N2(g) + O2(g) ⇄ 2 NO(g) contributes to air pollution whenever a fuel is...
The reaction N2(g) + O2(g) ⇄ 2 NO(g) contributes to air pollution whenever a fuel is burned in air at a high temperature, as in a gasoline engine. At 1500 K, Kc = 1.0×10-3. Suppose a sample of air has [N2] = 0.70 mol/L and [O2] = 0.20 mol/L before any reaction occurs. Calculate the equilibrium concentrations of reactants and products after the mixture has been heated to 1500 K. [N2] = M [O2] = M [NO] = M
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K...
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g); Kc = 5.6 ✕ 10−4 at 2098 K (a) What is the value of Kc for the reaction 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) at the same temperature? (b) What is the value of Kc for the reaction 1/2 N2(g) + 1/2 O2(g) equilibrium reaction arrow NO(g) at the same temperature? (c) Does the equilibrium in (a) favor the reactant or the products? reactant products (d) Does the equilibrium in...
The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.050. The reaction mixture...
The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.050. The reaction mixture starts with only the product, [NO] = 0.0300 M , and no reactants. Part A Find the equilibrium concentrations of N2 at equilibrium. Express your answer to two significant figures and include the appropriate units. [N2] = Part B Find the equilibrium concentrations of O2 at equilibrium. Part C Find the equilibrium concentrations of NO at equilibrium. Express your answer to two significant figures...
find equilibruim concentrations of O2, N2 and NO The reaction N2(g) + O2(g) = 2NO(g) is...
find equilibruim concentrations of O2, N2 and NO
The reaction N2(g) + O2(g) = 2NO(g) is carried out at a temperature at which Kc = 0.045. The reaction mixture starts with only the product, (NO) = 0.0300 M, and no reactants.
For the following equilibria, calculate the value of Kc and determine whether the equilibria exists mostly...
For the following equilibria, calculate the value of Kc and determine whether the equilibria exists mostly as reactants, as products or about equal amounts of both. All concentrations are at equilibrium. a) 2 NO(g) + O2(g) 2 NO2(g) [NO] = 0.0020 M, [O2] = 0.010 M, [NO2] = 0.100 M
3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2...
3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2 NH3(g) b) An equilibrium mixture at 500 K has the following concentrations: [N2] = 3.0 x 10-2 M [H2] = 3.7 x 10-2 M [NH3] = 1.6 x 10-2 M, calculate the equilibrium constant, Kc c) Calculate the Kp for this reaction d) Is the equilibrium mixture mostly reactants or products? e) Does this reaction go to nearly 100% completion? Explain f) If Qc...
The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3 at 2300...
The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3 at 2300 K. If the initial concentrations of N2 and O2 at 2300 K are both 1.58 M, what are the concentrations of NO when the reaction mixture reaches equilibrium? Concentrations of NO= UNITS If the initial concentrations of N2 and O2 at 2300 K are both 1.58 M, what are the concentrations of N2 when the reaction mixture reaches equilibrium? Concentrations of O2= If the...
Part B? Review | Constants Periodic Table H2NH3 Consider the following reaction: 2NH3(g) = N2(g) +...
Part B?
Review | Constants Periodic Table H2NH3 Consider the following reaction: 2NH3(g) = N2(g) + 3H2(g) Submit Previous Answers Correct The equilibrium constant is equal to the concentrations of the products divided by the concentrations of the reactants. The concentrations of both the reactants and the products are raised to a power of the respective coefficient from the balanced chemical reaction. K.= [N] [H] [NH3] Part B What is the numerical value of Kc for the reaction if the...
Please help i need to get these right in order to get an A PLEASE PLEASE...
Please help i need to get these right in order to get an A PLEASE PLEASE PLEASE 1. What is the Kc for the following reaction at equilibrium at 1000 ∘C if [CO]= 0.50 M , [H2]= 0.32 M , [CH4]= 1.6 M , and [H2O]= 2.8 M ? CO(g)+3H2(g)⇌CH4(g)+H2O(g) 2. The equilibrium constant, Kc, for the reaction of H2 and N2 is 1.7×102 at 225 ∘C. 3H2(g)+N2(g)←−→2NH3(g) If the system at equilibrium contains 0.19 M H2 and 0.026 M...
find equilibruim concentrations of O2, N2 and NO
The reaction N2(g) + O2(g) = 2NO(g) is carried out at a temperature at which Kc = 0.045. The reaction mixture starts with only the product, (NO) = 0.0300 M, and no reactants.
Part B?
Review | Constants Periodic Table H2NH3 Consider the following reaction: 2NH3(g) = N2(g) + 3H2(g) Submit Previous Answers Correct The equilibrium constant is equal to the concentrations of the products divided by the concentrations of the reactants. The concentrations of both the reactants and the products are raised to a power of the respective coefficient from the balanced chemical reaction. K.= [N] [H] [NH3] Part B What is the numerical value of Kc for the reaction if the...
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