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Vlad1618 [11]
3 years ago
7

How many molecules are in 28 grams of nitrogen gas in balloons?

Chemistry
1 answer:
melomori [17]3 years ago
6 0

Answer:

6.022\cdot 10^{23} molecules of nitrogen gas

Explanation:

In order to convert the mass of a given compound into the number of molecules, we need to:

  • identify the number of moles of a given compound dividing its mass by the molar mass, n = \frac{m}{M},
  • multiply the number of moles by the Avogadro's constant which tells us that 1 mole contains N_A = 6.022\cdot 10^{23} molecules.

In this problem:

m_{N_2} = 28~g

M_{N_2} = 28.01~g/mol

The number of particles is then found by:

N_{N_2} = n_{N_2}\cdot N_A = \frac{m_{N_2}}{M_{N_2}} N_A = \frac{28 g}{28.01 g/mol}\cdot 6.022\cdot 10^{23} mol^{-1} = 6.022\cdot 10^{23}

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7. Disulfur dichloride can be made by reacting chlorine gas with molten sulfur. What is the yield of S2Cl2 expected in a laborat
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Answer:

11.4g of S₂Cl₂ is the expected yield

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Explanation:

The reaction of sulfur S₈ with Cl₂ to produce S₂Cl₂ is:

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<em>Where 1 mole of sulfur reacts with four moles of chlorine to produce four moles of disulfur dichloride.</em>

To find the limiting reactant you need to convert mass of each reactant to moles using its molar mass, thus:

S₈ (Molar mass: 256.52g/mol): 10.0g ₓ (1mol / 256.52g) = 0.0390 moles S₈

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For a complete reaction of 0.0390 moles of sulfur, there are necessaries:

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As 4 moles of Cl₂ produce 4 moles of S₂Cl₂.<em> 0.0846 moles of Cl₂ produce, in theory, 0.0846 moles of S₂Cl₂ (Molar mass: 135.04g/mol). </em>In mass:

0.0846 moles S₂Cl₂ ₓ (135.04g/mol) =

<h3>11.4g of S₂Cl₂ is the expected yield</h3>

If you produce just the 85.0% of yield, mass of S₂Cl₂ is:

11.4g ₓ 85% =

<h3>9.69g of S₂Cl₂</h3>
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