Fall 2015 Quiz #2  [ENDORSED]

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Ivy Kwok 2I
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Joined: Wed Sep 21, 2016 2:58 pm

Fall 2015 Quiz #2

Postby Ivy Kwok 2I » Tue Oct 11, 2016 10:56 am

May someone explain the second part of #2 on the Fall 2015 practice quiz? I balanced the equation, converted the given quantities of Al and HCl to moles, and did some dimensional analysis, but I can't seem to get the correct answer. Thank you!

* Update: Aluminum and hydrogen chloride, HCl, react to form aluminum chloride in solution, AlCl3, and hydrogen gas. Balance the equation for this reaction. (I got 2 Al + 6 HCl => 2 AlCl3 + 3 H2.) If you had 5.43 g of aluminum and 7.80 g of hydrogen chloride, how many grams of AlCl3 would you get? *
Last edited by Ivy Kwok 2I on Tue Oct 11, 2016 5:21 pm, edited 1 time in total.

Chem_Mod
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Re: Fall 2015 Quiz #2

Postby Chem_Mod » Tue Oct 11, 2016 10:57 am

Remember to include the question itself in your post.

Megan Yabumoto 3K
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Re: Fall 2015 Quiz #2  [ENDORSED]

Postby Megan Yabumoto 3K » Wed Oct 12, 2016 12:33 am

In order to determine the amount of AlCl3 that will be produced, you will first need to determine which of the two reactants is the limiting reagent. Convert the given grams for each reactant to moles. Use these values to determine which is in the smaller quantity. Then, use the limiting reactant and plug into a dimensional analysis relationship to determine the amount of AlCl3 in grams produced.

Ivy Kwok 2I
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Joined: Wed Sep 21, 2016 2:58 pm

Re: Fall 2015 Quiz #2

Postby Ivy Kwok 2I » Wed Oct 12, 2016 9:36 pm

Thank you so much!


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