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oksian1 [2.3K]
3 years ago
15

Trace amounts of sulfur (S) in coal are burned in the presence of diatomic oxygen (O2) to form sulfur dioxide (SO2). Determine t

he minimum mass of oxygen required in the reactants and the mass of sulfur dioxide in the products when 1 kg of sulfur is burned.
Chemistry
1 answer:
Mashcka [7]3 years ago
3 0

Answer:

0.99 kg O₂

1.9 kg SO₂

Explanation:

Let's consider the reaction between sulfur and oxygen to form sulfur dioxide.

S + O₂ → SO₂

The mass ratio of S to O₂ is 32.07:32.00. The mass of oxygen required to react with 1 kg of sulfur is:

1 kg S × (32.00 kg O₂/32.07 kg S) = 0.998 kg O₂

The mass ratio of S to SO₂ is 32.07:64.07. The mass of sulfur dioxide formed when 1 kg of sulfur is burned is:

1 kg S × (64.07 kg SO₂/32.07 kg S) = 1.99 kg SO₂

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alukav5142 [94]

Answer:

5.56 × 10^23 molecules

Explanation:

The number of molecules in a molecule can be calculated by multiplying the number of moles in that molecule by Avagadro's number (6.02 × 10^23)

Using mole = mass/molar mass

Molar mass of N2O4 = 14(2) + 16(4)

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mole = 85.0/92

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number of molecules of N2O4 (nA) = 0.924 × 6.02 × 10^23

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