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29 Nov 2019

Given: The air pollutant NO is produced in automobile engines fromthe high-temperature reaction: N2(g)+O2(g)<=>2NO(g),Kc=1.7x10^-3. Question: Calculate the equilibrium concentrations ifthe initial concentrations are 2.31M N2 and 0.54M O2. (This N2/O2concentration ratio is the ratio found in air.)

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Elin Hessel
Elin HesselLv2
17 Dec 2019

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Related questions

TThe air pollutant NO is produced in automobile engines from the high-temperature reaction:

at 2300 K

If the initial concentrations of N2 and O2 at 2300 K are 2.24 M and 0.56 M, respectively, what are the concentrations of NO, N2, O2 when the reaction mixture reaches equilibrium?

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. Part A If the initial concentrations of N2 and O2 at 2300 K are both 1.50 M, what are the concentrations of NO when the reaction mixture reaches equilibrium? Express your answer to two significant figures and include the appropriate units.

Part B If the initial concentrations of N2 and O2 at 2300 K are both 1.50 M, what are the concentrations of N2 when the reaction mixture reaches equilibrium? Express your answer to three significant figures and include the appropriate units.

Part C If the initial concentrations of N2 and O2 at 2300 K are both 1.50 M, what are the concentrations of O2 when the reaction mixture reaches equilibrium? Express your answer to three significant figures and include the appropriate units.

1) The air pollutant NO is produced in automobile engines fromthe high-temperature reaction: N2(g)+O2(g)❝2NO(g) Kc=1.7Ý10❝3.

Calculate the equilibrium concentrations if the initialconcentrations are 2.24M N2 and 0.59M O2. (This N2/O2 concentrationratio is the ratio found in air.)

Express your answer using two significant figures. Enter youranswers numerically separated by commas.

2) At 700 K, Kp = 0.140 for the reactionClF3(g)?ClF(g)+F2(g).

Calculate the equilibrium partial pressures of ClF3, ClF, and F2if only ClF3 is present initially, at a partial pressure of 1.38atm.

Enter your answers numerically separated by commas.

3)In which of the following will the equilibrium shift to theproduct side under increased pressure by decreased volume?In whichof the following will the equilibrium shift to the product sideunder increased pressure by decreased volume?

C(s) + H2O(g) ? H2 (g) +CO(g)
CaCO3 (s) ? CaO(s) + CO2 (g)
Al2O3 (s) + 3H2 (g) ? 2Al(s) +3H2O(g)

2H2S(g) + SO2 (g) ? 3S(s) +2H2O(g)

4) When air is heated at very high temperatures in an automobileengine, the air pollutant nitric oxide is produced by thereaction

N2(g)+O2(g)?2NO(g),?H?=+182.6kJ
How does the equilibrium amount of NO vary with an increase intemperature?

When air is heated at very high temperatures in an automobileengine, the air pollutant nitric oxide is produced by thereaction
,
How does the equilibrium amount of vary with an increasein temperature?

amount of NO increases
amount of NO decreases

amount of NO remains the same

5) The equilibrium constant Kp for thereactionC(s)+H2O(g)???CO(g)+H2(g)
is 2.44 at 1000 K. The initial partial pressures are PH2O= 1.27atm , PCO = 1.03atm , and PH2 = 1.39atm.

a) What is the equilibrium partial pressure of H2O?

b) What is the equilibrium partial pressure of CO?

c) What is the equilibrium partial pressure of H2?

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