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How to use ICE tables
Posted: Thu Jan 10, 2019 1:29 pm
by Maayan Epstein 14B
How do I know what to plug into ice tables? For example, I know that I can plug in molarity to find initial, change, and equilibrium. Will this work for pressure too?
Thanks!
Re: How to use ICE tables
Posted: Thu Jan 10, 2019 2:39 pm
by Chem_Mod
Yes. Because, partial pressure in a gas reaction is essentially a way to represent concentration and you can use the ideal gas law to convert.
Re: How to use ICE tables
Posted: Thu Jan 10, 2019 5:54 pm
by Kevin ODonnell 2B
This table may help to visualize it all, and is an example that uses Molarity.
Re: How to use ICE tables
Posted: Sat Jan 12, 2019 4:38 pm
by Eruchi Okpara 2E
I'm still confused on how to find the change in molarity, can someone explain please? Does the number in front of the X come from the coefficient that is in front of the reactant or product?
Re: How to use ICE tables
Posted: Sat Jan 12, 2019 4:47 pm
by Michelle Wang 4I
Hi Eruchi,
In this situation we don't know the exact change in molarity that occurs in the reaction. We know that when the Cu(NH3)42+ dissociates, it forms 4 mol of NH3 and 1 mol of Cu2+. We use the stoichiometric coefficients of the balanced chemical equations to write the x that is added or taken away. That is why the 4NH3 has a +4x change in molarity.
Re: How to use ICE tables
Posted: Sat Jan 12, 2019 4:48 pm
by tierra parker 1J
Eruchi Okpara 2E wrote:I'm still confused on how to find the change in molarity, can someone explain please? Does the number in front of the X come from the coefficient that is in front of the reactant or product?
yes the coefficient of x is from the coefficients from the balanced equation. if the equilibrium concentration is given then you subtract the initial concentration from the equilibrium concentration