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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