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A chemistry problem set from morehouse college, focusing on molecular formulas, molar masses, mass of substances in solutions, balanced chemical equations, and mass percentages of elements in compounds. Students are required to calculate the mass of reagents needed to produce a certain mass of products for given chemical reactions.
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DUE: Friday, November 30, 2007
i. The molecular formula ii. The molar mass iii. The mass of substance in 50 mL of a 0.50 M solution of the compound.
a. Platinum(IV) chloride b. Table salt c. Hydrobromic acid
d. Acetic acid e. Potassium hydroxide f. Manganese(IV) oxide
a. C 5 H 10 O5(s) + O2(g) โ CO2(g) + H 2 O(g) b. S(s) + HNO3(aq) โ SO2(g) + NO(g) + H 2 O(l) c. Al 2 O3(s) + NaOH(aq) + H 2 O(l) โ NaAl(OH) 4 d. H 2 SO4(aq) + Na 2 CO3(aq) โ Na 2 SO4(aq) + H 2 O(l) + CO2(g) e. H2(g) + CO(g) โ C 8 H18(l) + H 2 O(l) f. NaOCl(aq) + NH3(aq) โ NaOH(aq) + NCl3(aq)
Wustite Hematite Magnetite % Iron --- --- --- % Oxygen 21.39 28.99 26.
a. What is the % composition of iron in each of the above oxides? b. Determine the empirical formula for each of the oxides of iron described above.
a. What is the mass percent copper in the unknown copper oxide? b. What is the empirical formula of the copper oxide? c. If water is produced as a byproduct in the above reaction, write a balanced chemical equation corresponding to this process. d. Based on your answer to part (c), calculate the mass of the copper oxide consumed when 2.5 L of hydrogen gas (initially at STP) are allowed to react completely to afford copper metal and water.