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April 24, 2014

April 24, 2014

Posted by **Michelle** on Tuesday, November 27, 2012 at 8:38pm.

Suppose you want to make 1.50 g of chromium (III) oxide, how many ml of 6.25M chromic acid will you need to use if the percent yield of the reaction is 68.6%?

- Chemistry -
**DrBob222**, Tuesday, November 27, 2012 at 9:35pmYou want 1.5 g Cr2O3 so the question you ask yourself is, "What number must I start with to get 1.5 g if the reaction is only 68.6% efficient?"

That's 0.686*X = 1.5 and X = 1.5/0.686 = about 2.3g or so but you should do this more accurately.

Then convert 2.3(actually the number you obtain) to mols.

mols Cr2O3 = 2.3g/molar mass Cr2O3.

Next, using the coefficients in the balanced equation, convert mols Cr2O3 to mols H2CrO4.

Finally, M H2CrO4 = mols H2CrO4/L H2CrO4. You have M and mols solve for L and convert to mL.

- Chemistry -
**Michelle**, Tuesday, November 27, 2012 at 10:24pmhow do I convert moles of Cr2O3 to moles of H2CrO4? I don't understand what this means

- Chemistry -
**DrBob222**, Wednesday, November 28, 2012 at 12:21amUse the coefficients in the balanced equation.

?mols Cr2O3 x (20 mols H2CrO4/10 mols Cr2O3)

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