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Chapter 4: Q73E (page 226)

Uranium can be isolated from its ores by dissolving it as UO2(NO3)2, then separating it as solid UO2(C2O4). Addition of 0.4031 g of sodium oxalate, NaC2O4, to a solution containing 1.481 g of uranyl nitrate, UO2(NO3)2, yields 1.073 g of solid

\(Na{C_2}{O_4} + U{O_2}{\left( {N{O_3}} \right)_2} + 3{H_2}O \to U{O_2}\left( {{C_2}{O_4}} \right) \cdot 3{H_2}O + 2NaN{O_3}\)

Short Answer

Expert verified

NaC2O4 is the limiting reactant.

The percent yield is 86.6 %.

Step by step solution

01

Balance chemical equation

Balance the chemical equation

02

Determine the molar mass

Find the molar mass.

1 mol =2(22.990) +2(12.011) +4(15.999) =133.998 g.

1mol= 238.029+8(15.999)+2(14.007) = 394.035 g.

1 mol = 238.029+9(15.999) +2(12.011) +6(1.008) = 412.09 g

03

Determine the yield

Find the theoretical yield

\(\begin{aligned}{}3.0083 \times {10^{ - 3}}\,mol\,Na{C_2}{O_4} \times \left( {\frac{{1\,mol\,U{O_2}\left( {{C_2}{O_4}} \right) \cdot 3{H_2}O}}{{1\,mol\,mol\,Na{C_2}{O_4}}}} \right) \times \\\left( {\frac{{412.09\,g\,U{O_2}\left( {{C_2}{O_4}} \right) \cdot 3{H_2}O}}{{1\,mol\,U{O_2}\left( {{C_2}{O_4}} \right) \cdot 3{H_2}O}}} \right)\\ = 1\,.239\,g\,U{O_2}\left( {{C_2}{O_4}} \right) \cdot 3{H_2}O\end{aligned}\)

Find the percent yield of

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Most popular questions from this chapter

In a laboratory experiment, the reaction of 3.0 mol of\({H_2}\)with 2.0 mol of\({I_2}\)produced 1.0 mol of HI. Determine the theoretical yield in grams and the percent yield for this reaction.

Indicate what type or types of reaction each of the following represents:

(a) \({H_2}O\left( g \right) + C\left( s \right) \to CO\left( g \right) + {H_2}\left( g \right)\)

(b) \(2KCl{O_3}\left( s \right) \to 2KCl\left( s \right) + 3{O_2}\left( g \right)\)

(c) \(Al{\left( {OH} \right)_3}\left( {aq} \right) + 3HCl\left( {aq} \right) \to AlC{l_3}\left( {aq} \right) + 3{H_2}O\left( l \right)\)

(d) \(Pb\left( {N{O_3}} \right)\left( {aq} \right) + {H_2}S{O_4}\left( {aq} \right) \to PbS{O_4}\left( s \right) + 2HN{O_3}\left( {aq} \right)\)

The principal component of mothballs is naphthalene, a compound with a molecular mass of about 130 amu, containing only carbon and hydrogen. A 3.000-mg sample of naphthalene burns to give 10.3 mg of CO2. Determine its empirical and molecular formulas.

The balanced molecular equations, write the complete ionic and net ionic equations for the following

(a)\({K_2}{C_2}{O_4}\left( {aq} \right) + Ba{\left( {OH} \right)_2}\left( {aq} \right) \to 2KOH\left( {aq} \right) + B{a_2}{C_2}{O_4}\)

(b)\(Pb{\left( {N{O_3}} \right)_2}\left( {aq} \right) + {H_2}S{O_4}\left( {aq} \right) \to PbS{O_4} + 2HN{O_3}\)

(c)\(CaC{O_3}\left( s \right) + {H_2}S{O_4}\left( {aq} \right) \to CaS{O_4} + C{O_2} + {H_2}O\)

Write a balanced molecular equation describing each of the following chemical reactions.

(a) Solid calcium carbonate is heated and decomposes to solid calcium oxide and carbon dioxide gas

(b)Gaseous butane reacts with diatomic oxygen gas to yield gaseous carbon dioxide and water vapor

(c)Aqueous solution of magnesium chloride and sodium hydroxide react to produce solid magnesium hydroxide and aqueous sodium chloride

(d) Water vapor reacts with sodium metal to produce solid sodium hydroxide and hydrogen gas.
See all solutions

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