Question

in the reaction A+B =C+D the concentration of A,B,C,D in moles/litre are 0.5,0.8,0.4,1.0 respectively the equilibrium constant is

Answer 1

Keq=[C][D]/[A][B]

Keq = 1.0x0.4/0.8x0.5
= 1.0

Answer 2

The equilibrium constant for the given reaction is 1.

Explanation:

Equilibrium constant in terms of concentration is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as $K_{eq}$

For a general chemical reaction:

$aA+bB\rightleftharpoons cC+dD$

The expression for $K_{eq}$ is written as:

$K_{eq}=\frac{[C]^c[D]^d}{[A]^a[B]^b}$

For the given chemical equation:

$A+B\rightleftharpoons C+D$

The expression of $K_{eq}$ for above equation is written as:

$K_{eq}=\frac{[C][D]}{[A][B]}$

We are given:

$[A]=0.5mol/L$

$[B]=0.8mol/L$

$[C]=0.4mol/L$

$[D]=1.0mol/L$

Putting values in above equation, we get:

$K_{eq}=\frac{0.4\times 1.0}{0.5\times 0.8}\\\\K_{eq}=1$

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