1A sample of PCl5gas is introduced into a flask at 250oC at a pressure of exactly 1 atm, but some of this gas decompose to PCl3and Cl2to produce an equilibrium total pressure of 1.98 atm. What is the value of the equilibrium constant, Kp, for this reaction?PCl5(g) PCl3(g) + Cl2(g)A) 50 atmB) 1.98 atmC) 48 atmD) 2.0 atm Partial pressure is proportional to moles and concentration, so you can work with partial pressures just like using moles or concentration.Construct the RICE table. Let x = partial pressure of PCl5that decomposes.Solve for x using the equilibrium total pressure.Substitute into the Kpexpression to find Kp.2PCl5(g) PCl3(g) + Cl2(g)1 atm0 0-x +x +x1 atm – x xx221121.981.9810.98(.98)48.02ppxKxxxxKatmOne equation in two unknowns, need another equation.The total final pressure was 1.98 atm.
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