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Inessa [10]
2 years ago
15

The reaction is: Fe2O3 (s) + 2Al (s) → 2Fe (l) + Al2O3 (s)

Chemistry
1 answer:
alukav5142 [94]2 years ago
4 0

There are 4.8 moles of Al2O3 produced when 2.4 mol of  Fe2O3 reacts with iron.

a)The equation of the reaction is;  Fe2O3 (s) + 2Al (s) → 2Fe (l) + Al2O3 (s)

From the reaction equation;

2 moles of Al produces 1 moles of Al2O3

x moles of Al produces 2.4 moles of Al2O3

x = 2 moles × 2.4 moles/1 moles

x = 4.8 moles

b) 1 mole of Fe2O3  produces 1 moles of  Al2O3

4.5 moles of Fe2O3  produces 4.5 moles of Al2O3

c) Number of moles in 3.6 g of Al = 3.6 g/27 g/mol = 0.133 moles

If 2 moles of Al yields 1 mole of Al2O3

0.133 moles Al yields 0.133 moles × 1 mole/ 2 moles

= 0.0665 moles

Mass of Al2O3 = 0.0665 moles × 102g/mol

= 6.8 g

d) Number of moles of iron =  3.6 g/56 g/mol = 0.064 moles

From the reaction equation;

1 mole of Al2O3 is produced when 2 moles of iron is produced

x moles of Al2O3 is produced when 0.064 moles is produced

x = 1 mole × 0.064 moles/ 2 moles

x = 0.032 moles

Mass of Al2O3 produced =  0.032 moles ×  102g/mol

= 3.3 g

Learn more: brainly.com/question/20339399

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A gaseous mixture composed of 20% CH4, 30% C2H4, 35% C2H2, and 15% C2H20. What is the average molecular weight of the mixture? a
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<u>Answer:</u> The correct answer is Option d.

<u>Explanation:</u>

We are given:

Mass percentage of CH_4 = 20 %

So, mole fraction of CH_4 = 0.2

Mass percentage of C_2H_4 = 30 %

So, mole fraction of C_2H_4 = 0.3

Mass percentage of C_2H_2 = 35 %

So, mole fraction of C_2H_2 = 0.35

Mass percentage of C_2H_2O = 15 %

So, mole fraction of C_2H_2O = 0.15

We know that:

Molar mass of CH_4 = 16 g/mol

Molar mass of C_2H_4 = 28 g/mol

Molar mass of C_2H_2 = 26 g/mol

Molar mass of C_2H_2O = 48 g/mol

To calculate the average molecular mass of the mixture, we use the equation:

\text{Average molecular weight of mixture}=\frac{_{i=1}^n\sum{\chi_im_i}}{n_i}

where,

\chi_i = mole fractions of i-th species

m_i = molar masses of i-th species

n_i = number of observations

Putting values in above equation:

\text{Average molecular weight}=\frac{(\chi_{CH_4}\times M_{CH_4})+(\chi_{C_2H_4}\times M_{C_2H_4})+(\chi_{C_2H_2}\times M_{C_2H_2})+(\chi_{C_2H_2O}\times M_{C_2H_2O})}{4}

\text{Average molecular weight of mixture}=\frac{(0.20\times 16)+(0.30\times 28)+(0.35\times 26)+(0.15\times 42)}{4}\\\\\text{Average molecular weight of mixture}=6.75

Hence, the correct answer is Option d.

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