Consider the reaction P4(g) → 2P2(g) where Kp = 1.00 × 10-1 at 1325 K. In an experiment where P4(g) was placed in a container at 1325 K, the equilibrium mixture of P4(g) and P2(g) has a total pressure of 1.00 atm. Calculate the equilibrium pressures of P4(g) and P2(g). Calculate the fraction (by moles) of P4(g) that has dissociated to reach equilibrium.
Answer to relevant QuestionsSuppose 1.50 atm of CH4(g), 2.50 atm of C2H6(g), and 15.00 atm of O2(g) are placed in a flask at a given temperature. The reactions are CH4(g) + 2O2(g) ⇌ CO2(g) + 2H2O(g) Kp = 1.0 × 104 2C2H6(g) + 7O2(g) ⇌ 4CO2(g) + ...At 207oC, Kp = 0.267 for the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) a. If 0.100 mole of PCl5(g) is placed in an otherwise empty 12.0-L vessel at 207oC, calculate the partial pressures of PCl5(g), PCl3(g), and Cl2(g) at ...A sample of gaseous nitrosyl bromide (NOBr) was placed in a container fitted with a frictionless, massless piston, where it decomposed at 25oC according to the following equation: 2NOBr(g) ⇌ 2NO(g) + Br2(g) The initial ...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 ...The specific heat capacity of silver is 0.24 JoC-1g-1. a. Calculate the energy required to raise the temperature of 150.0 g Ag from 273 K to 298 K. b. Calculate the energy required to raise the temperature of 1.0 mole of Ag ...
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