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AURORKA [14]
3 years ago
6

How to calculate the number of atoms, molecules, or ions

Chemistry
1 answer:
Leni [432]3 years ago
8 0
For atoms use a periodic table. The atomic number is the amount of atoms. For molecules and ions look up things revolved around the avogrados principle
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A teacher wants to figure out the amount of a solution that is needed for a titration experiment in a class lab. The class has 1
umka2103 [35]

Answer:

Im sure it's 1500 mL

Explanation:

You would have ti multiply by 15 i think

7 0
2 years ago
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Acetic acid (HC2H3O2) is the active ingredient in vinegar. Calculate the mass percent composition of O in acetic acid.
skelet666 [1.2K]

Answer:

53.29% of acetic acid is Oxygen

Explanation:

Step 1: Given data

Acetic acid it's molecular formula is HC2H3O2. This means it consists of 3 elements Carbon, Hydrogen and oxygen.

Step 2: the molar masses

The molecular mass of acetic acid is:

4* H = 4* 1.01 g/mole

2* C = 2*12 g/mole

2*O = 2* 16 g/mole

Total molar mass = 4+ 24+32 = 60.052 g/mole

Step 3: Calculate the mass percent

32 g of the 60.052 g is Oxygen

(32/60.052) *100% = 53.29%

53.29% of acetic acid is Oxygen.

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3 years ago
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A flashbulb of volume 1.70 mL contains O2(g) at a pressure of 2.30 atm and a temperature of 18.0°C. How many grams of O2(g)
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Answer:

0.0001637 mol

Explanation:

PV = nRT

Very important formula in chem

2.3 atm * 0.0017 L = n * 0.082057 * 291 K

= 0.0001637 mol O2

This concept is very important in chem, practice it.

7 0
3 years ago
Does respiratory happens in the lungs true or false?
Anna007 [38]

Answer:

True

Explanation:

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2 years ago
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A 0.334 g sample of an unknown compound occupies 245 ml at 298 K and 1.22 atm. What is the molar mass of the unknown compound.
marysya [2.9K]

Answer:

27.4 g/mol

Explanation:

Assuming the compound is a gas and that it behaves ideally, we can solve this problem by using the <em>PV=nRT formula</em>, where:

  • P = 1.22 atm
  • V = 245 mL ⇒ 245 mL / 1000 = 0.245 L
  • n = ?
  • R = 0.082 atm·L·mol⁻¹·K⁻¹
  • T = 298 K

<u>Inputting the data</u>:

  • 1.22 atm * 0.245 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 298 K

<u>Solving for n</u>:

  • n = 0.0122 mol

With the <em>calculated number of moles and given mass</em>, we <u>calculate the molar mass</u>:

  • 0.334 g / 0.0122 mol = 27.4 g/mol
6 0
2 years ago
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