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In an analysis of interhalogen reactivity, 0.500 mol of
Chapter 17, Problem 43P(choose chapter or problem)
Problem 43P
In an analysis of interhalogen reactivity, 0.500 mol of ICl was placed in a 5.00-L flask, where it decomposed at a high T: 2ICl(g) ⇌ I2(g) + Cl2(g). Calculate the equilibrium concentrations of I2, Cl2, and ICl (Kc= 0.110 at this temperature).
Questions & Answers
QUESTION:
Problem 43P
In an analysis of interhalogen reactivity, 0.500 mol of ICl was placed in a 5.00-L flask, where it decomposed at a high T: 2ICl(g) ⇌ I2(g) + Cl2(g). Calculate the equilibrium concentrations of I2, Cl2, and ICl (Kc= 0.110 at this temperature).
ANSWER:
Solution 43P:
Here, we are going to calculate the equilibrium concentration of I2, Cl2, and ICl.
Step 1:
Given reaction,
2ICl(g) ⇌ I2(g) + Cl2(g)
Volume = 5.0 L
Moles of ICl(g) =0.500 mol
Therefore, initial [ICl] = =0.1 M
Let be the concentration of I2(g) and Cl2(g) are formed after some time. With change in time the concentration of ICl(g) will be reduced by -2x.
Therefore,
At change, [ICl] = , [I2] =
and [Cl2] =
Thus,
At equilibrium,
[ICl] = , [I2] =
and [Cl2] =
Hence, the reaction table for the reaction is given below:
