Question

1 mole = 6.02 x 10²3 particles. Particles can be: ____ or ____ or ____ or _____.

1 mole 22.4 Lat STP. Liter is a measure of ______.

1 mole = Formula mass in grams. Formula mass uses ________ to calculate.

2-step mole problems: have ___ _____ in the question.

1-step mole problems: have _______ in the question.

1. How many moles are in 25.0g of 0₂? 2. How many particles are in 100.0g of gold? M
3. How many liters are in 3 moles of carbon dioxide?
4. How many particles are in 50.0L of NO₂?
5. How many grams are in 5.0 x 1025 molecules of water?
6. How many grams are on 6.00 moles of C5H₁205?
7. How many moles are in 22.4L of H₂S? 8. How many moles are in 3.00 x 1022 atoms of gold?
9. How many particles are in 25.0g of C? 10. How many liters are in 20.0 moles of CO₂?
11. How many grams are in 44.8L of oxygen?
12. How many liters are in 1.34g of CO? to calculate.​

Answer 1

1 mole = 6.02 x 10²³ particles. Particles can be: atoms, molecules, ions, or formula units.

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1 mole = 22.4 L at STP. Liter is a measure of volume.

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1 mole = Formula mass in grams. Formula mass uses the atomic masses of elements to calculate.

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2-step mole problems: have moles and a conversion factor in the question.

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1-step mole problems: have either moles, grams, particles, or liters in the question.

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1. To find the number of moles in 25.0g of O₂, we use the formula:

Moles = Mass / Molar mass

The molar mass of O₂ is 32 g/mol.

Moles = 25.0g / 32 g/mol = 0.78125 mol

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2. To find the number of particles in 100.0g of gold, we use the formula:

Particles = Moles * Avogadro's number

The molar mass of gold (Au) is 197 g/mol.

Moles = 100.0g / 197 g/mol ≈ 0.5076 mol

Particles = 0.5076 mol * 6.02 x 10²³ particles/mol ≈ 3.06 x 10²³ particles

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3. To find the number of liters in 3 moles of carbon dioxide (CO₂) at STP, we use the fact that 1 mole of any gas occupies 22.4 L at STP.

Liters = 3 moles * 22.4 L/mol = 67.2 L

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4. To find the number of particles in 50.0L of NO₂, we use the formula:

Particles = Moles * Avogadro's number

First, we need to find the number of moles. Since the volume is given, we convert it to moles using the ideal gas law.

Moles = Volume / 22.4 L/mol = 50.0L / 22.4 L/mol ≈ 2.23 mol

Particles = 2.23 mol * 6.02 x 10²³ particles/mol ≈ 1.34 x 10²⁴ particles

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5. To find the number of grams in 5.0 x 10²⁵ molecules of water (H₂O), we use the formula:

Grams = Moles * Molar mass

The molar mass of water (H₂O) is 18 g/mol.

Moles = (5.0 x 10²⁵ molecules) / (6.02 x 10²³ molecules/mol) ≈ 8.31 mol

Grams = 8.31 mol * 18 g/mol ≈ 149.58 g

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6. To find the number of grams in 6.00 moles of C₅H₁₂O₅, we use the formula:

Grams = Moles * Molar mass

The molar mass of C₅H₁₂O₅ is 92.1 g/mol.

Grams = 6.00 mol * 92.1 g/mol = 552.6 g

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7. To find the number of moles in 22.4L of H₂S, we use the formula:

Moles = Volume / 22.4 L/mol = 22.4L / 22.4 L/mol = 1 mol

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8. To find the number of moles in 3.00 x 10²² atoms

of gold, we use the formula:

Moles = Number of atoms / Avogadro's number

Moles = (3.00 x 10²² atoms) / (6.02 x 10²³ atoms/mol) ≈ 0.498 mol

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9. To find the number of particles in 25.0g of carbon (C), we use the formula:

Moles = Mass / Molar mass

The molar mass of carbon (C) is 12 g/mol.

Moles = 25.0g / 12 g/mol ≈ 2.08 mol

Particles = 2.08 mol * 6.02 x 10²³ particles/mol ≈ 1.25 x 10²⁴ particles

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10. To find the number of liters in 20.0 moles of carbon dioxide (CO₂) at STP, we use the fact that 1 mole of any gas occupies 22.4 L at STP.

Liters = 20.0 moles * 22.4 L/mol = 448 L

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11. To find the number of grams in 44.8L of oxygen (O₂) at STP, we use the fact that 1 mole of any gas occupies 22.4 L at STP and the molar mass of oxygen is 32 g/mol.

Moles = Volume / 22.4 L/mol = 44.8L / 22.4 L/mol = 2 mol

Grams = 2 mol * 32 g/mol = 64 g

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12. To find the number of liters in 1.34g of carbon monoxide (CO), we use the fact that 1 mole of any gas occupies 22.4 L at STP and the molar mass of carbon monoxide is 28 g/mol.

Moles = Mass / Molar mass = 1.34g / 28 g/mol ≈ 0.048 mol

Liters = 0.048 mol * 22.4 L/mol ≈ 1.08 L