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Juliette [100K]
3 years ago
12

2) write down two examples of mixturesand state their use in daily life.​

Chemistry
1 answer:
prisoha [69]3 years ago
7 0

Answer:

<em>first </em><em>example</em><em> </em><em>is</em><em>. </em><em>Air </em><em> </em><em>it </em><em>is </em><em>mixture </em><em>of </em><em>many </em>

<em>gases </em><em> </em>

<em>it's </em><em>us </em><em> </em><em>it </em><em>keeps </em><em>us </em><em>alive </em><em> </em><em>and </em><em>many </em><em>more </em><em>uses</em>

<em>second </em><em>example</em><em> </em><em>is </em><em>water </em><em>is </em><em>also </em><em>a </em><em>mixture</em><em> </em>

<em>made </em><em>up </em><em>of </em><em>carbon </em><em>and </em><em>hydrogen</em><em> </em>

<em>and </em><em>its uses </em><em>is </em><em>to </em><em>fulfill</em><em> </em><em>our </em><em>needs </em>

<em>hope </em><em>it </em><em>helps</em>

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3 years ago
An iron ore sample weighing 0.5562 g is dissolved HCl (aq), and the iron is obtained as Fe2 in solution. This solution is then t
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Answer:

\% Fe^{+2}=70%

Explanation:

Hello,

In this case, we could considering this as a redox titration:

Fe^{+2}+(Cr_2O_7)^{-2}\rightarrow Fe^{+3}+Cr^{+3}

Thus, the balance turns out (by adding both hydrogen ions and water):

Fe^{+2}\rightarrow Fe^{+3}+1e^-\\(Cr_2^{+6}O_7)^{-2}+14H^++6e^-\rightarrow 2Cr^{+3}+7H_2O\\\\6Fe^{+2}+(Cr_2^{+6}O_7)^{-2}+14H^++6e^-\rightarrow Cr^{+3}+7H_2O+6Fe^{+3}+6e^-

Thus, by stoichiometry, the grams of Fe+2 ions result:

m_{Fe^{+2}}=0.04021\frac{molK_2Cr_2O_7}{L}*0.02872L*\frac{6molFe^{+2}}{1molK_2Cr_2O_7}*\frac{56gFe^{+2}}{1molFe^{+2}}=0.388gFe^{+2}

Finally, the mass percent is:

\% Fe^{+2}=\frac{0.388g}{0.5562g}*100\%\\  \% Fe^{+2}=70%

Best regards.

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