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balu736 [363]
2 years ago
8

A chemist reacted 17.25 grams of sodium metal with an excess amount of chlorine gas. The chemical reaction that occurred is show

n. Na + Cl2 → NaCl If the percentage yield of the reaction is 88%, what is the actual yield? Show your work, including the use of stoichiometric calculations and conversion factors.​
Chemistry
1 answer:
Afina-wow [57]2 years ago
3 0

<u>Answer:</u> The actual yield of the product is 38.57 g

<u>Explanation:</u>

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}} ......(1)

We are given:

Given mass of Na = 17.25 g

Molar mass of Na = 23 g/mol

Putting values in equation 1, we get:

\text{Moles of Na}=\frac{17.25g}{23g/mol}=0.75mol

For the given chemical reaction:

2Na+Cl_2\rightarrow 2NaCl

By stoichiometry of the reaction:

2 moles of Na produces 2 moles of NaCl

So, 0.75 moles of Na will produce = \frac{2}{2}\times 0.75=0.75mol of NaCl

We know, molar mass of NaCl = 58.44 g/mol

Putting values in above equation, we get:

\text{Mass of NaCl}=(0.75mol\times 58.44g/mol)=43.83g

The percent yield of a reaction is calculated by using an equation:

\% \text{yield}=\frac{\text{Actual value}}{\text{Theoretical value}}\times 100 ......(1)

Given values:

Percent yield of the product = 88 %

Theoretical value of the product = 43.83 g

Plugging values in equation 1:

88\% =\frac{\text{Actual yield}}{43.83g}\times 100\\\\\text{Actual yield}=\frac{88\times 43.83}{100}=38.57g

Hence, the actual yield of the product is 38.57 g

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This is defined as the mole of solute per unit litre of solution. Mathematically, it can be expressed as:

Molarity = mole / Volume

<h3>How to determine the mole of NiCl₂•6HO₂</h3>
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Mole = Molarity × Volume

Mole of NiCl₂•6HO₂ = 0.035 × 0.5

Mole of NiCl₂•6HO₂ = 0.0175 mole

<h3>How to determine the mass of NiCl₂•6HO₂</h3>
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Mass = mole × molar mass

Mass of NiCl₂•6HO₂ = 0.0175 × 238

Mass of NiCl₂•6HO₂ = 4.165 g

Thus, 4.165 g of NiCl₂•6HO₂ is needed to prepare the solution

Learn more about molarity:

brainly.com/question/15370276

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