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Katarina [22]
2 years ago
15

2 C4H10 + 13O2 -------> 8CO2 + 10H2O

Chemistry
1 answer:
ANEK [815]2 years ago
4 0

Answer:

A. 2 : 13

B. 10 : 13

C. 10 moles of water, H₂O.

D. 2 moles of butane, C₄H₁₀

E. 116 g of butane, C₄H₁₀

F. 13 moles of oxygen, O₂

G. 416 g of oxygen, O₂

Explanation:

The equation for the reaction is given below:

2C₄H₁₀ + 13O₂ —> 8CO₂ + 10H₂O

A. Determination of the mole ratio between butane and oxygen gas.

Mole of butane, C₄H₁₀ = 2 moles

Mole of oxygen, O₂ = 13 moles

Mole ratio of butane and oxygen = 2 : 13

B. Determination of the mole ratio between water and oxygen gas

Mole of the water, H₂O = 10 moles

Mole of oxygen, O₂ = 13 moles

Mole ratio of water and oxygen = 10 : 13

C. Determination of the moles of water formed.

From the balanced equation above,

10 moles water, H₂O were produced.

D. Determination of the moles of butane burned.

From the balanced equation above,

2 moles of butane, C₄H₁₀ were burned.

E. Determination of the mass of butane burned.

Molar mass of C₄H₁₀ = (12×4) + (10×1)

= 48 + 10 = 58 g/mol

Mole of C₄H₁₀ = 2 moles

Mass of C₄H₁₀ =?

Mass = mole × molar mass

Mass of C₄H₁₀ = 2 × 58

Mass of C₄H₁₀ = 116 g

Thus, 116 g of butane, C₄H₁₀ were burned.

F. Determination of the number of mole of oxygen used.

From the balanced equation above,

13 moles of oxygen, O₂ were used.

G. Determination of the mass of oxygen used.

Molar mass of O₂ = 2 × 16 = 32 g/mol

Mole of O₂ = 13 moles

Mass of O₂ =?

Mass = mole × molar mass

Mass of O₂ = 13 × 32

Mass of O₂ = 416 g

Thus, 416 g of oxygen, O₂ were used.

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Explanation:

For point a:  

Actual\ yield = 6.52 \ kg\\\\Percent \ yield= 66\%\\\\Percent \ yield = \frac{Actual \ yield}{Theoretical\ yield} \times 100 \%\\\\Theoretical\ yield \ of \ MnO_2 = \frac{Actual \ yield}{Percent \ yield} \times 100\%\\\\=\frac{6.52 \ kg}{66 \%} \times 100\% =9.88 \ kg\\\\

Equation:  

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Calculating the amount of MnCO_3

= 9.88 \ kg \times \frac{1000 \ g}{1 \ kg} \times \frac{1 \ mol \ MnO_2}{86.94 \ g} \times \frac{2 \ Mol \ MnCO_3}{2 \ mol \ MnO_2} \times \frac{114.95\ g}{1 \ mol \ MnCO_3 }\times \frac{1\ kg}{1000\ g}\\\\=  13.1 \ kg

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Actual\ yield = 4.0 \ kg\\\\Percent\ yield=97.0\%\\\\Percent \ yield = \frac{Actual \ yield}{Theoretical \ yield} \times 100 \% \\\\Theoretical \ yield\  of\  Mn = \frac{Actual \ yield}{Percent \ yield} \times 100\%\\\\

=\frac{4.0 \ kg}{97.0\%} \times 100\% =4.12 \ kg

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3MnO_2 +4AL \longrightarrow 3Mn + 2AL_2O_3\\\\

Calculating the amount of MnO_2:  

= 4.12 \ kg \times \frac{1000 \ g}{1 \ kg} \times \frac{1 \ mol \ Mn}{54.94 \ g} \times \frac{3 \ Mol \ MnO_2}{3 \ mol \ Mn} \times \frac{86.94 \ g}{1 \ mol \ MnO_2 }\\\\=  6516 \ g \\\\=6.52 \ kg\\\\

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