## 6th Edition Ch11 Question 1d

Netpheel Wang 4L
Posts: 60
Joined: Fri Sep 28, 2018 12:15 am

### 6th Edition Ch11 Question 1d

Q: True or False
If one starts with higher concentrations of reactants, the equilibrium concentrations of the products will be larger

What is the difference between equilibrium concentrations and partial pressure?

Albert Duong 4C
Posts: 66
Joined: Fri Sep 28, 2018 12:17 am
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### Re: 6th Edition Ch11 Question 1d

I believe it is due to Le Chatelier's principle (we haven't learned this yet in class, but it may be familiar from high school) where, for example, if the reactant concentration decreases, the equilibrium shifts in the direction of the reactants to restore balance, resulting in more reactants being formed (thus, less products are formed). In this case, with a higher concentration of reactants, the concentration of products increases because the equilibrium shifts in the direction of products to balance out the increased concentration of reactants.

Shally Li 2C
Posts: 30
Joined: Fri Sep 28, 2018 12:22 am

### Re: 6th Edition Ch11 Question 1d

If you increase the concentration of reactants, it will form more product, however this doesn't mean that the concentration of product will be greater than the concentration of reactants at equilibrium.

Partial pressure is the pressure exerted by a gas in a mixture and is expressed in atm, bar, Torr, etc. Concentration is the is amount of solute per amount of solution and can be expressed using molarity (mol/L).

marisaimbroane1J
Posts: 69
Joined: Fri Sep 28, 2018 12:23 am

### Re: 6th Edition Ch11 Question 1d

Concentration is measured in moles/L whereas partial pressure is in a unit such as atm (I know units are not included in the K expression, but that is how you can identify each of them). Partial pressure is basically how much of the total pressure the product/reactant is and can only be used when all reactants and products are gases.