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Consider the following reaction: 1₂(g) + Cl₂(g) 21C1(g), K₂ = 81.9 (at 25°C) A reaction mixture at 25°C initially contains Pt₂ = 0.200 atm, Pcl₂ = 0.200 atm, and Pic=0.00 atm. ▾ Part A Find the equilibrium partial pressure of I2 at this temperature. Express the pressure to three decimal places and include the appropriate units. R₂ = Submit Part B Set up an ICE (Initial, Change, Equilibrium) table using a variable (e.g., z) to determine an expression that defines the partial pressures of the reactants and product at equilibrium. Once you solve for x, use it to calculate the partial pressure of I₂ at equilibrium. No credit lost. Try again. PC₁, = Submit Value Part C Find the equilibrium partial pressure of Cl₂ at this temperature. Express the pressure to three decimal places and include the appropriate units. Previous Answers Request Answer PA Submit atm Value 4 → ⒸIE Previous Answers Request Answer Pa = Value atm µA 4 X Incorrect; Try Again Set up an ICE (Initial, Change, Equilibrium) table using a variable (e.g., z) to determine an expression that defines the partial pressures of the reactants and product at equilibrium. Once you solve for x, use it to calculate the partial pressure of Cl₂ at equilibrium. ? Find the equilibrium partial pressure of ICI at this temperature. Express the pressure to three decimal places and include the appropriate units. Review | Constants | Periodic Table ? atm O IB ? Previous Answers Request Answer X Incorrect; Try Again Set up an ICE (Initial, Change, Equilibrium) table using a variable (e.g., z) to determine an expression that defines the partial pressures of the reactants and product at equilibrium. Once you solve for x, use it to calculate the partial pressure of IC] at equilibrium.