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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 0.042 at a certain temperature. If 2.860 g of PCI, initially decomposes in a 700 mL closed container, what will the equilibrium concentration of PCI, be? PCI, (g) PCl3(g) + Cl₂(g) = < PREV 1 NEXT > Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. Kc = 2 [2x]² [2.860+x] [2x] [2.860 -x] [0.01374-2x [0.01962+x] [0.01962-x] [0.01962- 2x [4.086 +x] 3 = 0.042 RESET [2.860-2x] [0.01374+x] [0.01374-x] [4.086-x] [4.086-2x]
Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 0.042 at a certain temperature. If 2.860 g of PCI, initially decomposes in a 700 mL closed container, what will the equilibrium concentration of PCI, be? PCIs(g) PCl3(g) + Cl₂(g) 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. Initial (M) Change (M) Equilibrium (M) 0 2.860+x 2.860 x - 0.01962-2x 4.086 +x 1 PCI, (g) 2.860 0.01374 0.01374 + x 4.086 - 2x 2.860- 2x 4.086-x 2 PCI, (g) + 0.01962 Cl₂(g) 4.086 0.01374-x 0.01374-2x 0.01962+x +X RESET -X 0.01962-x
0 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 0.042 at a certain temperature. If 2.860 g of PCI, initially decomposes in a 700 mL closed container, what will the equilibrium concentration of PCI, be? PCIs(g) PCI3(g) + Cl₂(g) < PREV Based on your ICE table and expression for Kc, solve for the concentration of PCI, at equilibrium. M 1 [PCIs] eq = 2 3 0.01457 0.02913 0.01960 0.01883 7.908 x 10-4 RESET 0.00505