Limiting Reactant Calculations  [ENDORSED]

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Kevin Hernandez 3A
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Joined: Fri Sep 29, 2017 7:06 am

Limiting Reactant Calculations

Postby Kevin Hernandez 3A » Fri Dec 08, 2017 12:51 am

20. How many moles of CO2(g) are produced when 1 kg of CaCO3(s) is used to neutralize an acid spill? The equation for the reaction at 1 atm and 25 degrees C is:

CaCO3(s) + H2SO4(aq) ---> CaSO4(s) + CO2(g) + H2O(l)

How do we know that CaCO3 is the limiting reagent?

Jessica Nunez 1I
Posts: 58
Joined: Thu Jul 13, 2017 3:00 am

Re: Limiting Reactant Calculations

Postby Jessica Nunez 1I » Fri Dec 08, 2017 1:14 pm

I think we would need to assume CaCO3 is the limiting reactant based on what the problem tells us. If we had to find the limiting reactant, I believe they would give us the mass for both reactants.

Kevin Liu 3G
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Joined: Fri Sep 29, 2017 7:07 am

Re: Limiting Reactant Calculations  [ENDORSED]

Postby Kevin Liu 3G » Sat Dec 09, 2017 3:57 pm

Based off of the question, they are trying to clean up the acid H2SO4(aq) so it is safe to assume there would be more acid than the substance used to neutralize the spill. If they tell you the mass of both substances you would convert it to moles and go from there to find the limiting reactant.

Gianna Graziano 1A
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Joined: Wed Apr 04, 2018 3:00 am

Re: Limiting Reactant Calculations

Postby Gianna Graziano 1A » Wed Apr 04, 2018 11:39 am

The question is asking you for the amount of moles of CO2 that are produced and you can assume that CaCO3 is the limiting reactant since it is what is being used to neutralize the acid spill. After you calculate the molar mass of CaCO3(approximately 10 moles), you look at the ratio between CaCO3 and CO2. Since there is a 1:1 ratio, you know 10 moles of CaCO3 produces 10 moles of CO2.


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