4 posts • Page 1 of 1
If the coefficient isn't 1, then you would have something such as -2x (if the coefficient is 2). Then make sure to still square the value when you put it in the equilibrium constant equation (it would be (2x)^2-- so 4x^2).
Molar ratios will affect the way in which you proceed with your ICE table since, for example, not all reactions use up all of the reactants to form a product. If, for instance, a balanced chemical reaction produces 1 mole of product for every 2 moles of reactant, the concentration of the reactant will decrease by X amount (-X), which will produce twice that amount of product (+2x). Be mindful of the stoichiometric coefficients of the reaction when formatting your ICE table.
Who is online
Users browsing this forum: No registered users and 2 guests