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. Calculate the...
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.
Calculate the equilibrium concentrations if the initial concentrations are 2.28 M N2 and 0.56 M O2. (This N2/O2concentration ratio is the ratio found in air.)
Express your answer using two significant figures. Enter your answers numerically separated by commas.
Homework Answers
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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.
Calculate the...
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...
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...
Problem 7: Nitric oxide, NO, is a common air pollutant produced by automobile engines and power...
Problem 7: Nitric oxide, NO, is a common air pollutant produced by automobile engines and power plants according to the reaction N2 (g)+02 (g) 2NO (g) A constant-volume reactor of 100 L is initially charged with 4 mol of N2 and 1 mol of O2 and then temperature is increased to 800 K. Estimate the equilibrium extent of the reaction if the pressure is kept constant at 1 bar (Answer: 5.567 x 10-6)
The reaction below is carried out at a different temperature at which Kc=0.055. This time, however,...
The reaction below is carried out at a different temperature at which Kc=0.055. This time, however, the reaction mixture starts with only the product, [NO]=0.0100M [NO]=0.0100M, and no reactants. Find the equilibrium concentrations of N2, O2, and NO at equilibrium. N2(g)+O2(g)⇌2NO(g) Express your answers to three significant figures separated by commas.
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 reaction N2(g) + O2(g) 2NO(g), Kc = 4.0 at a particular temperature. In a 1.0-L...
For the reaction N2(g) + O2(g) 2NO(g), Kc = 4.0 at a particular temperature. In a 1.0-L container, 1.0 mol of N2 and O2 are mixed. Determine the concentration of NO once equilibrium is reached at the given temperature. =________ Please explain so I understand
Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reaction $$N2(g)+O2(g)2NO(g) At...
Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reaction $$N2(g)+O2(g)2NO(g) At 2000.0°C Kc = 4.100 × 10–4 and ΔH° = 180.6 kJ. 1st attempt What is the value of Kc at 43.00°C?
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
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each...
Consider the following reaction: A(g)⇌B(g)+C(g) Find the equilibrium concentrations of A, B, and C for each of the following different values of Kc. Assume that the initial concentration of A in each case is 1.0 M and that the reaction mixture initially contains no products. Make any appropriate simplifying assumptions. Part A Kc= 1.8 Express your answer using two significant figures. Enter your answers numerically separated by commas. [A][ A ], [B], [C] = nothing M
QUESTION 12 BEE [CLO-6] At 2000 °C, the equilibrium constant for the reaction: 2NO(g) N2(g) +...
QUESTION 12 BEE [CLO-6] At 2000 °C, the equilibrium constant for the reaction: 2NO(g) N2(g) + O2(g) Is Kc = 2.4. Knowing that the initial concentration of NO is 0.175 M, what will be the concentrations of NO, N2 and O2 at equilibrium? [Hint: you have to build a table to find the answer) (0.175), +2x, +2x (0.175), +x, +x +x (0.175-2x), +x, (0.175-x), +x, +X
Problem 7: Nitric oxide, NO, is a common air pollutant produced by automobile engines and power plants according to the reaction N2 (g)+02 (g) 2NO (g) A constant-volume reactor of 100 L is initially charged with 4 mol of N2 and 1 mol of O2 and then temperature is increased to 800 K. Estimate the equilibrium extent of the reaction if the pressure is kept constant at 1 bar (Answer: 5.567 x 10-6)
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.
QUESTION 12 BEE [CLO-6] At 2000 °C, the equilibrium constant for the reaction: 2NO(g) N2(g) + O2(g) Is Kc = 2.4. Knowing that the initial concentration of NO is 0.175 M, what will be the concentrations of NO, N2 and O2 at equilibrium? [Hint: you have to build a table to find the answer) (0.175), +2x, +2x (0.175), +x, +x +x (0.175-2x), +x, (0.175-x), +x, +X
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