The following reaction was performed in a sealed vessel at 783 ∘C∘C : H2(g)+I2(g)⇌2HI(g)H2(g)+I2(g)⇌2HI(g) Initially, only H2 & I2 were present at concentrations of [H2]=3.35M & [I2]=3.00M. The equilibrium concentration of I2's 0.09 M . What's the equilibrium constant, Kc, for the reaction at this temperature?
The equilibrium constant, K�, of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium.
For a gaseous reaction with the general form: aA+bB⇌cC+dD
the Kc and Kp expressions are given by:
Kc=[C]c[D]d/ [A]a[B] b
Kp=(PC)c(PD)d/(PA)a(PB)b
The subscript cc or pp indicates whether K is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved since their composition does not change throughout the reaction. The standard state of a pure substance is the pure substance itself, and although the quantity may change the sample remain pure. The constant value is incorporated into the value of K, and does not need to be accounted for separately.
The following reaction was performed in a sealed vessel at 783 ∘C∘C :
H2(g)+I2(g)⇌2HI(g)H2(g)+I2(g)⇌2HI(g)
Initially, only H2 & I2 were present at concentrations of [H2]=3.35M & [I2]=3.00M. The equilibrium concentration of I2's 0.09 M . What's the equilibrium constant, Kc, for the reaction at this temperature?
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