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Calculate the following at equilibriumEquation: A(g)+B(g)=C(g)+D(g)  Keq=49 One mole...

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Calculate the following at equilibrium

Equation: A(g)+B(g)=C(g)+D(g)  Keq=49

One mole of C and D are added to a .5L container.

Also what will happen to the value of the equilibrium constant if the temperature increased?

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For the reaction A(g)+B(g)=C(g)+D(g) the value of the equilibrium constant is Keq=49.

Keq = ({C}{D})/({A}*{B}) = 49

As one mole of C and D are added to a 0.5 l container, the concentration of each of them is 2 mol/l

49 = (2*2)/({A}*{B})

=> {A}*{B} = 4/49

As per the chemical equation the concentration of A and B would be the same. This gives the concentration of A and B equal to 2/49 mol/l

It is not possible to say how an increase in temperature will influence the equilibrium constant as for exothermic reactions an increase in temperature decreases the equilibrium constant while for endothermic reactions the equilibrium constant increases as the temperature is increased.

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