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juin [17]
3 years ago
10

Consider the balanced chemical reaction below and determine the percent yield for iron if 11.2 moles of Iron(III) oxide yielded

17.4 moles of iron
Fe2O3+3CO>2Fe+3CO2
Chemistry
1 answer:
gayaneshka [121]3 years ago
8 0

Answer:

The yield percent is 77.68%

Explanation:

Fe_{2}O_{3}+3CO\longrightarrow2Fe+3CO_{2}

1 mole of Fe_{2}O_{3} yields 2 moles of Fe.

So, 11.2 moles of Iron(III) oxide must yield 22.4 moles of Fe theoretically. This is according to the balanced equation.

Theoretical Yield = 22.4 moles of Fe

Experimental Yield = 17.4 moles of Fe

Yield\:Percentage=\frac{Experimental\:Yield}{Theoretical\:Yield}\times100\\\\Yield\:Percentage=\frac{17.4}{22.4}\times100=77.68\%

Therefore, the yield percent is 77.68%

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Answer:

D

Explanation:

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Compound X has a molar mass of 416.48 g mol
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Answer:

P₂Cl₁₀

Explanation:

From the question given above, the following data were obtained:

Molar mass of compound X = 416.48 g/mol

Percentage of phosphorus (P) = 14.87%

Percentage of Chlorine (Cl) = 85.13%

Molecular formula of X =?

Next, we shall determine the empirical formula of compound X. This can be obtained as follow:

P = 14.87%

Cl = 85.13%

Divide by their molar mass

P = 14.87 / 31 = 0.480

Cl = 85.13 / 35.5 = 2.398

Divide by the smallest

P = 0.480 / 0.480 = 1

Cl = 2.398 / 0.480 = 5

Empirical formula of compound X is PCl₅

Finally, we shall determine the molecular formula of compound X. This can be obtained as follow:

Molar mass of compound X = 416.48 g/mol

Empirical formula = PCl₅

Molecular formula =?

Molecular formula= [Empirical formula]ₙ

[PCl₅]ₙ = 416.48

[31 + (35.5 × 5)]ₙ = 416.48

[31 + 177.5]n = 416.48

208.5n = 416.48

Divide both side by 208.5

n = 416.48 / 208.5

n = 2

Molecular formula = [PCl₅]ₙ

Molecular formula = [PCl₅]₂

Molecular formula = P₂Cl₁₀

Therefore, the molecular formula of compound X is P₂Cl₁₀

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