In this lab, we'll be synthesizing an Fe oxalate using (NH4)2Fe(SO4)2· 6 H2O. The formula of the

the grams of the K -2 or the K -3 rather or the mass of the potassium trioxyl -latoferate 3. So

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the grams of the K -2 or the K -3 rather or the mass of the potassium trioxyl -latoferate 3. So

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In this lab, we'll be synthesizing an Fe oxalate using \( \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Fe}\left(\mathrm{SO}_{4}\right)_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O} \). The formula of the Fe oxalate you synthesize will be in the form of \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot n \mathrm{H}_{2} \mathrm{O} \), where \( n \) could be 1,2 , or 3 . Calculate the molar masses of \( \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Fe}\left(\mathrm{SO}_{4}\right)_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O} \) and the three possible Fe oxalates \( \left(\mathrm{FeC}_{2} \mathrm{O}_{4} \cdot n \mathrm{H}_{2} \mathrm{O}\right) \). a. \( \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Fe}\left(\mathrm{SO}_{4}\right)_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O} \) : \( \square \) \( \mathrm{g} \mathrm{mol}^{-1} \) b. \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot \mathrm{H}_{2} \mathrm{O} \) : \( \square \) \( \mathrm{g} \mathrm{mol}^{-1} \) c. \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O} \) : \( \square \) \( \mathrm{g} \mathrm{mol}^{-1} \) d. \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot 3 \mathrm{H}_{2} \mathrm{O} \) : \( \square \) \( \mathrm{g} \mathrm{mol}^{-1} \)

          In this lab, we'll be synthesizing an Fe oxalate using \( \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Fe}\left(\mathrm{SO}_{4}\right)_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O} \). The formula of the Fe oxalate you synthesize will be in the form of \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot n \mathrm{H}_{2} \mathrm{O} \), where \( n \) could be 1,2 , or 3 .

Calculate the molar masses of \( \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Fe}\left(\mathrm{SO}_{4}\right)_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O} \) and the three possible Fe oxalates \( \left(\mathrm{FeC}_{2} \mathrm{O}_{4} \cdot n \mathrm{H}_{2} \mathrm{O}\right) \).
a. \( \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Fe}\left(\mathrm{SO}_{4}\right)_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O} \) : \( \square \) \( \mathrm{g} \mathrm{mol}^{-1} \)
b. \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot \mathrm{H}_{2} \mathrm{O} \) : \( \square \) \( \mathrm{g} \mathrm{mol}^{-1} \)
c. \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot 2 \mathrm{H}_{2} \mathrm{O} \) : \( \square \) \( \mathrm{g} \mathrm{mol}^{-1} \)
d. \( \mathrm{FeC}_{2} \mathrm{O}_{4} \cdot 3 \mathrm{H}_{2} \mathrm{O} \) : \( \square \) \( \mathrm{g} \mathrm{mol}^{-1} \)

In this lab, we'll be synthesizing an Fe oxalate using (NH4)2Fe(SO4)2· 6 H2O. The formula of the Fe oxalate you synthesize will be in the form of FeC2O4· n H2O, where n could be 1,2 , or 3 .

Calculate the molar masses of (NH4)2Fe(SO4)2· 6 H2O and the three possible Fe oxalates (FeC2O4· n H2O).
a. (NH4)2Fe(SO4)2· 6 H2O : □ gmol^-1
b. FeC2O4·H2O : □ gmol^-1
c. FeC2O4· 2 H2O : □ gmol^-1
d. FeC2O4· 3 H2O : □ gmol^-1

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