ChemBytes - Chapter 7

Answers

1. The equilibrium constants for the following reactions have been measured at 823K: CoO(s) + H₂(g) Co(s) + H₂O(g)         K₁ = 67
   CoO(s) + CO(g) Co(s) + CO₂(g)         K₂ = 490 From these data, calculate the equilibrium constant of the following reaction at 823K: CO₂(g) + H₂(g) CO(g) + H₂O(g)        K₃ = ? K₃ = 0.137
2. Solid ammonium carbamate, NH₄COONH₂, dissociates completely into ammonia and carbon dioxide when it evaporates, as shown by the following equation: NH₄COONH₂(s) 2 NH₃(g) + CO₂(g) At 25°C, the total pressure of the gases in equilibrium with the solid is 0.116 atm. What is the equilibrium constant of the reaction? If 0.10 atm of CO₂ is introduced after equilibrium is reached, will the final pressure of CO₂ be greater, less than, or equal to 0.1 atm? Will the pressure of NH₃ increase, decrease, or stay the same? K_equil = 2.3x10^-4; final pressure of CO₂ > 0.1 atm; Pressure NH₃ will decrease
3. The gaseous compound NOBr decomposes according to the reaction NOBr(g) NO(g) + 1/2 Br₂(g) At 350K, the equilibrium constant K_p is equal to 0.15. If 0.50 atm of NoBr, 0.40 atm of NO, and 0.20 atm of Br₂ are mixed at this temperature, will any net reaction occur? If so, will Br₂ be consumed or formed? A reaction occurs and Br₂ is consumed
4. 4. Would you expect the equilibrium constant for the following reaction to increase, decrease, or stay the same as the temperature increases? Why? I₂(g) 2I(g) K_equil increases with temperature.