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The dissociation of molecular iodine into iodine atoms is represented as I2(g) ⇌ 2I(g) At 1000 K, the equilibrium constant Kc for the reaction is 3.80 × 10−5. Suppose you start with 0.0460 mol of I2 in a 2.33−L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of I2?   M What is the equilibrium concentration of I?   M

Question

 
The dissociation of molecular iodine into iodine atoms is represented as
 

I2(g) ⇌ 2I(g)

 
At 1000 K, the equilibrium constant Kc for the reaction is 3.80 

×

 10−5. Suppose you start with 0.0460 mol of I2 in a 2.33−L flask at 1000 K. What are the concentrations of the gases at equilibrium?
 
What is the equilibrium concentration of I2?
 

 

 M
 
What is the equilibrium concentration of I?
 

 

 M

check_circleAnswer
Step 1

The Kc expression for given reaction is shown below,

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Step 2

The initial concentration of I2 ...

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