For a gaseous reaction: A + 2B <---> 2C, increasing pressure from 10 to 20 bar will increase the products formation

The effect of pressure on the equilibrium of a gaseous reaction is determined by the change in the number of moles of gas in the reaction. In the given reaction: A + 2B <---> 2C, the number of moles of gas on both sides of the reaction is the same (3 moles on both sides). Therefore, according to Le Chatelier's principle, which states that a system at equilibrium will adjust to counteract any change in conditions, an increase in pressure will not favor the formation of products or reactants. The system will remain at equilibrium. So, increasing the pressure from 10 to 20 bar will not increase the formation of the products in this case.