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shutvik [7]
3 years ago
7

0.329 M copper (II) nitrate was reacted with 0.528 M potassium carbonate as follows: Cu (NO subscript 3 )subscript 2 italic (a q

italic )space plus space straight K subscript 2 CO subscript 3 italic (a q italic )rightwards arrow CuCO subscript 3 italic (s italic )space plus space 2 thin space KNO subscript 3 italic (a q italic )Determine the percent yield if 163.9 mL of each reactant were allowed to react, and a mass of 4.883 g of solid were obtained.
Chemistry
1 answer:
EastWind [94]3 years ago
3 0

Answer:

73.33% is the percent yield

Explanation:

Percent yield is defined as:

Actual yield (4.883g) / Theoretical yield * 100

Based on the reaction:

Cu(NO₃)₂(aq) + K₂CO₃(aq) → CuCO₃(s) + 2KNO₃(aq)

<em>1 mole of copper nitrate reacts per mol of potassium carbonate.</em>

<em />

To solve this question we must find limiting reactant. With limiting reactant we can find the theoretical moles of solid produced and its mass as follows:

<em>Moles Cu(NO₃)₂:</em>

0.1639L * (0.329mol / L) = 0.0539 moles

<em>Moles K₂CO₃:</em>

0.1639L * (0.528mol / L) = 0.0865 moles

As the reaction is 1:1, the limiting reactant is Cu(NO₃)₂.

1 mol of Cu(NO₃)₂ produces 1 mol of CuCO₃. That means theoretical moles produced are 0.0539 moles. And the mass is:

<em>Mass CuCO₃ -Molar mass: 123.55g/mol-</em>

0.0539 moles * (123.55g / mol) = 6.659g of CuCO₃ is the theoretical mass

And percent yield:

4.883g / 6.659g * 100

<h3>73.33% is the percent yield</h3>
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