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iris [78.8K]
3 years ago
7

What volume of SO2 is produced when 2.35 g of sulfur burns? (All volumes are measured at STP) S (s) + O2(g) →SO2(g)

Chemistry
1 answer:
azamat3 years ago
7 0

1.64 L of SO₂ is produced when 2.35 g of Sulfur burns.

<u>Explanation:</u>

First of all, we need to write the balanced equation as,

S (s) + O₂ (g) → SO₂ (g)

Now we have to find the number of moles of sulfur by using its given mass and molar mass.

1 mol of Sulfur atoms = 32 g of sulfur

Now the given mass is 2.35 g.

So $\frac{2.35}{32} = 0.073 mol

1 mol of S produces 1 mol of SO₂.

So 0.073 mol of S produces 0.073 mol of SO₂.

At STP, 1 mol of SO₂ occupies a volume of 22.4 L.

0.073 mol of SO₂ occupies a volume of 22.4 × 0.073 = 1.64 L

So 1.64 L of SO₂ is produced.

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Explanation:

To convert from liters to moles, divide by 22.4:

35.88 L / 22.4 = 1.602 moles CO

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What is the pH of 0.000134 M solution of HCI?
mafiozo [28]

Answer: The pH will be 3.87

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

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According to stoichiometry,

1 mole of HCl gives 1 mole of H^+

Thus 0.000134 moles of HCl gives =\frac{1}{1}\times 0.000134=0.0001342 moles of H^+

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5 0
3 years ago
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Answer:

I got the answers but it won't let me post it correctly on here....

Explanation:

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