How to Solve Stoichiometry Problems Involving Mass and Balanced Equations?

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Discussion Overview

The discussion revolves around solving a stoichiometry problem involving mass and balanced chemical equations. Participants explore the steps necessary to determine the mass of magnesium nitrate produced from a given mass of aluminum nitrate based on a balanced reaction.

Discussion Character

  • Homework-related

Main Points Raised

  • One participant presents a stoichiometry problem involving the reaction between aluminum nitrate and magnesium, expressing uncertainty about how to begin solving it.
  • Another participant suggests converting the mass of aluminum nitrate into moles as a first step to solve the problem.
  • A participant reports converting grams of aluminum nitrate to approximately 0.2539 moles but remains confused about the next steps.
  • There is a discussion about using the mole ratio from the balanced equation to find the relationship between moles of aluminum nitrate and magnesium nitrate.
  • Participants clarify that the mole ratio is 2 moles of aluminum nitrate to 3 moles of magnesium nitrate.
  • One participant seeks guidance on how to apply the mole ratio to the calculated moles of aluminum nitrate.
  • A later reply indicates that dimensional analysis can be used to set up the calculation for the mass of magnesium nitrate produced.
  • Finally, one participant confirms they arrived at the correct answer after the discussion.

Areas of Agreement / Disagreement

The discussion reflects a lack of consensus on the specific steps to take after converting grams to moles, with participants providing varying levels of guidance and clarification. However, the final participant indicates they found the solution, suggesting some resolution for that individual.

Contextual Notes

Participants express uncertainty about the application of mole ratios and dimensional analysis, indicating potential gaps in understanding the steps involved in stoichiometric calculations.

Who May Find This Useful

Students seeking assistance with stoichiometry problems, particularly those involving mass and balanced equations, may find this discussion helpful.

GLprincess02
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Homework Statement



Given the balanced equation 2Al(NO3)3 + 3Mg ==> 3Mg(NO3)2 + 2Al , if 54.1 g of aluminum nitrate is reacted, what mass of magnesium nitrate is produced?

2. The attempt at a solution
I've been given an entire packet dedicated to stoichiometry, but nothing in here covers this problem. I am unsure of how to even begin solving it. Maybe if I had help with the first few steps I could solve the rest.
 
Last edited:
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a good way to go about this problem is to convert the mass of aluminum nitrate into moles of aluminum nitrate, then you can figure out how many moles of magnesium (do you mean aluminum or magnesium nitrate) were produced.
 
Ok so I converted the grams of aluminum nitrate into moles and got approx. 0.2539 moles. I'm still confused about what to do next, though.
 
Last edited:
GLprincess02 said:
Ok so I converted the grams of aluminum nitrate into moles and got approx. 0.2539 moles. I'm still confused about what to do next, though.

Now you need to use the mole fraction, which you get from the balanced reaction.
 
What is the mole fraction? Like, 2 moles of aluminum nitrate to 3 moles of magnesium nitrate?
 
GLprincess02 said:
What is the mole fraction? Like, 2 moles of aluminum nitrate to 3 moles of magnesium nitrate?

Yes.
(2mol Al nitrate/3mol Mg nitrate)
 
Ok, so how do I use this ratio in relation to the 0.2539 moles of aluminum nitrate? I guess I still don't really get all of the steps.
 
GLprincess02 said:
Ok, so how do I use this ratio in relation to the 0.2539 moles of aluminum nitrate? I guess I still don't really get all of the steps.

It is a dimensional analysis setup

mol Al nitrate(mole fraction)(convert mol Mg nitrate to g)=soln
 
So I take 0.2539 and multiply it by 2/3 first, right?
 
  • #10
Never mind, I got the right answer. Thanks for the help. :)
 

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