ICE tables

Moderators: Chem_Mod, Chem_Admin

Posts: 61
Joined: Fri Sep 28, 2018 12:15 am

ICE tables

Postby haleyervin7 » Thu Jan 17, 2019 12:21 am

How does an ICE table change when the stoichiometric coefficient isn't 1?

Posts: 69
Joined: Fri Sep 28, 2018 12:23 am

Re: ICE tables

Postby marisaimbroane1J » Thu Jan 17, 2019 9:57 am

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).

Posts: 60
Joined: Fri Sep 28, 2018 12:28 am

Re: ICE tables

Postby KatrinaPho_2I » Thu Jan 17, 2019 11:17 am

The stoichiometric coefficients will be the same coefficients that you put in the "change" part of the table. If the coefficient is 1, the change will be =/- x. If the coefficient is 3, the change will be =/- 3x.

Courtney Quan 1C
Posts: 60
Joined: Fri Sep 28, 2018 12:26 am
Been upvoted: 2 times

Re: ICE tables

Postby Courtney Quan 1C » Thu Jan 17, 2019 11:18 am

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.

Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 5 guests