The equilibrium constant for a reaction, often denoted as K, is a measure of the ratio of the concentrations of products to reactants at equilibrium. It is important to note that the equilibrium constant K is dependent on temperature but not on pressure.

This is because the equilibrium constant K is derived from the standard Gibbs free energy change, ΔG°, for the reaction, which is a function of temperature only.

Therefore, the equilibrium constant at 20 bar and 150 C would still be 0.38, the same as it was at 10 bar and 150 C.

However, it's important to note that while the equilibrium constant itself does not change with pressure, the position of equilibrium (i.e., the actual concentrations of A, B, and C at equilibrium) can change with pressure. This is due to Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

In this case, increasing the pressure would shift the equilibrium position to the side with fewer moles of gas to reduce the pressure, if the total moles of gas on each side are different.

Question

The equilibrium constant for a reaction, often denoted as K, is a measure of the ratio of the concentrations of products to reactants at equilibrium. It is important to note that the equilibrium constant K is dependent on temperature but not on pressure.

This is because the equilibrium constant K is derived from the standard Gibbs free energy change, ΔG°, for the reaction, which is a function of temperature only.

Therefore, the equilibrium constant at 20 bar and 150 C would still be 0.38, the same as it was at 10 bar and 150 C.

However, it's important to note that while the equilibrium constant itself does not change with pressure, the position of equilibrium (i.e., the actual concentrations of A, B, and C at equilibrium) can change with pressure. This is due to Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

In this case, increasing the pressure would shift the equilibrium position to the side with fewer moles of gas to reduce the pressure, if the total moles of gas on each side are different.

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The equilibrium constant for a reaction, often denoted as K, is a measure of the ratio of the concentrations of products to reactants at equilibrium. It is important to note that the equilibrium constant K is dependent on temperature but not on pressure.

This is because the equilibrium constant K is derived from the standard Gibbs free energy change, ΔG°, for the reaction, which is a function of temperature only.

Therefore, the equilibrium constant at 20 bar and 150 C would still be 0.38, the same as it was at 10 bar and 150 C.

However, it's important to note that while the equilibrium constant itself does not change with pressure, the position of equilibrium (i.e., the actual concentrations of A, B, and C at equilibrium) can change with pressure. This is due to Le Chatelier's principle, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

In this case, increasing the pressure would shift the equilibrium position to the side with fewer moles of gas to reduce the pressure, if the total moles of gas on each side are different.

For a gaseous reaction: A + 2B <---> 2C, the reaction equilibrium constant at 150 C and 10 bar is 0.38. What could be the equilibrium constant at 20 bar and 150 C?

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