Question

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?