A 2.20 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 32.0 percent of the NOCl had dissociated: 2NOCl(g) 2NO(g) + Cl2(g) Calculate the equilibrium constant Kc for the reaction.
A 2.20 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 32.0 percent of the NOCl had dissociated: 2NOCl(g) 2NO(g) + Cl2(g) Calculate the equilibrium constant Kc for the reaction.
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A 2.20 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 32.0 percent of the NOCl had dissociated:
2NOCl(g) 2NO(g) + Cl2(g)
Calculate the equilibrium constant Kc for the reaction.
Expert Solution
Step 1
Given datas ;
2NOCl(g) ----> 2NO(g) + Cl2(g)
We have 2.20 mol NOCI in a 1.50 L container at 400°C and after equilibrium, NOCI is 32 % dissociated.
&
We have to find the equilibrium constant Kc.
Firstly ,
Molarity of NOCl
= 2.20 mol / 1.50 L
= 1.466 mol/L or 1.466 M
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