At 1000 K the N2(g) and O2(g) in air (78% N2, 21% O2, by moles) react to form a mixture of NO(g) and NO2(g). The values of the equilibrium constants are 1.5 × 10-4 and 1.0 × 10-5 for the formation of NO(g) and NO2(g), respectively. At what total pressure will the partial pressures of NO(g) and NO2(g) be equal in an equilibrium mixture of N2(g), O2(g), NO(g), and NO2(g)?
Answer to relevant QuestionsThe equilibrium constant Kp for the reaction CCl4(g) ⇌ C(s) + 2Cl2(g) at 700oC is 0.76. Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700oC. A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g) ⇌ X(g) + Y(g) A 2.00- g sample of XY (molar mass = 165 g/ mol) is placed in a container with a movable piston at 25oC. The pressure is ...The overall reaction in a commercial heat pack can be represented as 4Fe(s) + 3O2(g) → 2Fe2O3(s) ΔH = –1652 kJ a. How much heat is released when 4.00 moles of iron is reacted with excess O2? b. How much heat is released ...Explain how calorimetry works to calculate ΔH or ΔE for a reaction. Does the temperature of the calorimeter increase or Decrease for an endothermic reaction? How about for an exothermic reaction? Explain why ΔH is ...Consider an airplane trip from Chicago, Illinois, to denver, Colorado. List some path-Dependent functions and some state functions for the plane trip.
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