6th Edition Ch11 Question 1d

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Netpheel Wang 4L
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6th Edition Ch11 Question 1d

Postby Netpheel Wang 4L » Mon Jan 07, 2019 8:40 pm

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

Why is the answer true?

What is the difference between equilibrium concentrations and partial pressure?

Albert Duong 4C
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Re: 6th Edition Ch11 Question 1d

Postby Albert Duong 4C » Mon Jan 07, 2019 8:50 pm

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
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Re: 6th Edition Ch11 Question 1d

Postby Shally Li 2C » Mon Jan 07, 2019 8:52 pm

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
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Re: 6th Edition Ch11 Question 1d

Postby marisaimbroane1J » Mon Jan 07, 2019 8:53 pm

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.


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