Problem: For the reaction system      H2(g) + X2(g) ⇌ 2 HX(g)Kc = 24.4 at 300 K. If the reaction is set up with the following initial concentrations, what will the equilibrium concentration of X2 be? initial H2 = 0.150 M          initial X2 = 0.200 M          initial HX = 0.600 MA. 0.0365 M B. 0.114 M C. 0.164 M D. 0.0730 ME. 0.500 M

FREE Expert Solution

We are being asked to calculate the equilibrium concentration of X2 for the given equilibrium reaction:

   H2(g) + X2(g) ⇌ 2 HX(g)            Kc = 24.4 at 300 K. 


When dealing with equilibrium and Kc:

Kc → equilibrium units are in molarity 
Kc is an equilibrium expression:

Kc=productsreactants

only aqueous and gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the concentrations in the equilibrium expression


Given:    


Initial Concentrations:

initial H2 = 0.150 M          

initial X2 = 0.200 M         

initial HX = 0.600 M



Let’s calculate the Reaction Quotient (Q) using the given initial concentration to determine which direction the equilibrium will proceed:

Q=productsreactants

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Problem Details

For the reaction system      H2(g) + X2(g) ⇌ 2 HX(g)
Kc = 24.4 at 300 K. If the reaction is set up with the following initial concentrations, what will the equilibrium concentration of X2 be? 

initial H2 = 0.150 M          initial X2 = 0.200 M          initial HX = 0.600 M

A. 0.0365 M 

B. 0.114 M 

C. 0.164 M 

D. 0.0730 M

E. 0.500 M

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