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hw L1

Posted: Thu Jul 11, 2019 2:30 am
by D-nice1D
Hi I'm really confused on how they want me to go about this


Without using a calculator, estimate what amount of Br2
(in moles) can be obtained from 0.30 mol ClO2 in the reaction
6 ClO21g2  2 BrF31l2 S 6 ClO2F1s2  Br21l2

Re: hw L1

Posted: Thu Jul 11, 2019 7:42 am
by hannabarlow1A
How you wrote out the chemical equation is a bit confusing, but in general, you can tell how many moles are being produced based on the ratios between the stoichiometric coefficients. For example, if there the stoichiometric coefficient for ClO2 is 6 and the stoichiometric coefficient for Br2 is 1, then there are 6 moles of ClO2 for every 1 mole of Br2. If they give you the exact amount of moles for one, you can then figure out the other based on their ratio.

Re: hw L1

Posted: Mon Sep 30, 2019 1:49 pm
by Esha Chawla 2E
Hi! This is how I would go about solving this problem:

Since we are only given that there is 0.30 mole of ClO2, we can assume that there is enough BrF3 for the reaction. Thus, for the purposes of this problem, we assume that the 0.30 mole of ClO2 is our limiting reactant.

Next, we should check to see if the equation is balanced. If you go through and check every atom, you will find that the equation is balanced.

To actually determine the mount of Br2 produced, look at the stoichiometric coefficients. You see that for every 6 moles of ClO2, there is 1mole of Br2. Using this, you can set up the following equation:

(0.30 moles of ClO2) * (1 mol Br2/6 moles ClO2)

You can see that the 'moles of ClO2' will cancel out, leaving you with how many moles of Br2 should be produced. You're answer should come out to 0.050 moles of Br2.