NH4COONH2(s)<-> 2NH3(g) + CO2(g). If equilibrium pressure is 3 atm for the above reaction; Kp will be :
Correct answer: A. 4
- A. 4
- B. 27
- C. 4/27
- D. 1/27
Explanation
To find the equilibrium constant Kp for the reaction NH4COONH2(s) <-> 2NH3(g) + CO2(g), we use the formula Kp = PNH3^2 * PCO2 where P represents the partial pressures of the gases. Given that the total equilibrium pressure is 3 atm, and considering the stoichiometry of the reaction (2:1 for NH3 to CO2), we can determine that PNH3 = 2 atm and PCO2 = 1 atm. Thus, Kp = (2)^2 * (1) = 4. The other options result from errors in calculating the partial pressures or applying the equilibrium expression.
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Thermochemistry measures energy changes in chemical reactions and distinguishes exothermic from endothermic processes. Work covers systems, surroundings and state functions, internal energy, the first law of thermodynamics, enthalpy and Hess's law, including the sign conventions used when heat enters or leaves a system.
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