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Helga [31]
3 years ago
9

Suppose an aqueous solution containing 1.25 g of lead(II) acetate is treated with 5.95 g of carbon diox- ide. Calculate the theo

retical yield of lead carbonate.
Chemistry
1 answer:
8_murik_8 [283]3 years ago
8 0

Answer:

1.02 g is the theoretical yield for PbCO₃

Explanation:

The reaction is

Pb(CH₃COO)₂  +  CO₂  + H₂O  →  PbCO₃ +  2CH₃COOH

1 mol of  lead(II) acetate react with 1 mol of carbon dioxide and 1 mol of water toproduce 1 mol of lead(II) carbonate and 2 moles of acetic acid.

With the two mass of the reactants, let's find put the limiting reactant.

1.25 g / 325.29 g/mol = 3.84×10⁻³ moles

5.95 g / 44 g/mol = 0.135 moles

Certainly, the limiting reactant is the lead(II) acetate. Ratio is 1:1, so if I have 0.135 moles of dioxide, I need the same amount of acetate. I only have 3.84×10⁻³ moles, that's why this is the limiting reactant.

Ratio is 1:1 too, with the lead(II) carbonate so 3.84×10⁻³ moles of acetate would produce 3.84×10⁻³ moles of carbonate.

Let's convert the moles to mass:

3.84×10⁻³ mol .  267.2 g/ mol = 1.02 g

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The amount left after 20 years = 154.15 mg

<h3>Further explanation </h3>

The atomic nucleus can experience decay into 2 particles or more due to the instability of its atomic nucleus.  

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The decay formula for isotope :

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Then for t=20 years, the amount left :

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If 125.0g of nitrogen is reacted with 125.0g of hydrogen, what is the theoretical yield of the reaction? What is the excess reac
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Answer:

Hydrogen is the excess reactant

Nitrogen is the limiting reactant

151.6g is theoretical yield

Explanation:

The reaction of N₂ with H₂ to produce NH₃ is:

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To find theoretical yield we need to determine limiting reactant with the moles of each gas as follows:

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4.46 moles N2 * (3moles H2 / 1mol N2) = 13.38 moles of hydrogen

As there are 62.5 moles of hydrogen:

<h3>Hydrogen is the excess reactant</h3><h3>Nitrogen is the limiting reactant</h3><h3 />

With nitrogen, the limiting reactant, we determine theoretical moles (Assuming 100% of the reaction occurs) and theoretical yield (In mass):

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8.92 moles of ammonia * (17g/mol) =

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