Given:
Molar mass of CO2 = 44.01g/mol
3.21x10^25 molecules of CO2
Required:
Mass of CO2
Solution:
Avogadro’s number states that
for every mole of atom, there are 6.023x10^23 units of atom. The units may be
formula units, atoms. In here, you need to divide 3.21x10^25 molecules of CO2
to 6.023x10^23 molecules per mole.
3.21x10^25 molecules of CO2 / 6.023x10^23
molecules per mole = 53.30 moles CO2
53.30 moles CO2 (44.01g/mol CO2)
= 2346 g of CO2
Scratch Test is your answer
A scratch test is when one rubs a mineral on a piece of white tile, and sees what color is left behind. Also, the mineral that has the scratches is weaker than the material that leaves the scratch mark.
hope this helps
<h3>Answer:</h3>
100 g O₂
<h3>General Formulas and Concepts:</h3>
<u>Math</u>
<u>Pre-Algebra</u>
Order of Operations: BPEMDAS
- Brackets
- Parenthesis
- Exponents
- Multiplication
- Division
- Addition
- Subtraction
<u>Chemistry</u>
<u>Atomic Structure</u>
<u>Stoichiometry</u>
- Using Dimensional Analysis
<h3>Explanation:</h3>
<u>Step 1: Define</u>
[RxN - Balanced] CH₄ + 2O₂ → CO₂ + 2H₂O
[Given] 2 mol CH₄
[Solve] x g O₂
<u>Step 2: Identify Conversions</u>
[RxN] 1 mol CH₄ → 2 mol O₂
[PT] Molar Mass of O - 16.00 g/mol
Molar Mass of O₂ - 2(16.00) = 32.00 g/mol
<u>Step 3: Stoichiometry</u>
- Set up conversion:
- Multiply/Divide:
<u>Step 4: Check</u>
<em>Follow sig fig rules and round. We are given 1 sig fig.</em>
128 g O₂ ≈ 100 g O₂
Answer:
CuSO4(aq)
Explanation:
The aqueous for of CuSO₄ is an electrolyte and it will conduct electricity.
CuSO₄ is an ionic substance and in solid state, it will not have the ability to conduct electricity.
- In aqueous form, it will contain free mobile ions which serves as carriers of electric current.
- In the solid state, the ions are arranged into a crystal lattice and will not conduct a current of electricity.
- The remaining given compounds will not conduct electricity as they are non-polar and do not have free mobile electrons.
