A sample of gaseous PCl5 was introduced into an evacuated flask so that the pressure of pure PCl5 would be 0.50 atm at 523 K. However, PCl5 decomposes to gaseous PCl3 and Cl2, and the actual pressure in the flask was found to be 0.84 atm. Calculate Kp for the decomposition reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) at 523 K. Also calculate K at this temperature.
Answer to relevant QuestionsA sample of S8(g) is placed in an otherwise empty, rigid container at 1325 K at an initial pressure of 1.00 atm, where it decomposes to S2(g) by the reaction S8(g) ⇌ 4S2(g) At equilibrium, the partial pressure of S8 is ...At 900oC, Kp = 1.04 for the reaction CaCO3(s) ⇌ CaO(s) + CO2(g) At a low temperature dry ice (solid CO2), calcium oxide, and calcium carbonate are introduced into a 50.0- L reaction chamber. The temperature is raised to ...At 35oC, K = 1.6 × 10-5 for the reaction 2NOCl(g) ⇌ 2NO(g) + Cl2(g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.0 moles of pure NOCl in a 2.0- L flask b. ...How will the equilibrium position of a gas- phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does ...At 25° C, Kp < 1 × 10-31 for the reaction N2(g) + O2(g) ⇌ 2NO(g) a. Calculate the concentration of NO (in molecules/ cm3) that can exist in equilibrium in air at 25oC. In air PN2 = 0.8 atm and PO2 = 0.2 atm. b. Typical ...
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