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answerhappygod
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Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as I₂(g) = 21(g) At 1000 K, the equilibrium constant K for the reaction is 3.80 × 10-5. Suppose you start with 0.0451 mol of I₂ in a 2.34-L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of 1₂? M What is the equilibrium concentration of I? M
Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as I₂(g) = 21(g) At 1000 K, the equilibrium constant K for the reaction is 3.80 × 10-5. Suppose you start with 0.0451 mol of I₂ in a 2.34-L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of 1₂? M What is the equilibrium concentration of I? M
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