<h3>
Answer:</h3>
5.00 mol 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>
- Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.<u>
</u>
<u>Stoichiometry</u>
- Using Dimensional Analysis
<h3>
Explanation:</h3>
<u>Step 1: Define</u>
3.01 × 10²⁴ atoms O₂
<u>Step 2: Identify Conversions</u>
Avogadro's Number
<u>Step 3: Convert</u>
- Set up:
- Multiply/Divide:
<u>Step 4: Check</u>
<em>Follow sig fig rules and round. We are given 3 sig figs.</em>
4.99834 mol O₂ ≈ 5.00 mol O₂
Answer:
V₂ = 60 cm³
Explanation:
According to Charle's Law, "Volume of given amount of gas is directly proportional to applied temperature at constant pressure". Mathematically,
V₁ / T₁ = V₂ / T₂ ---- (1)
Data Given:
V₁ = 30 cm³
T₁ = 10 °C = 10 + 273 = 283 K
V₂ = ?
T₂ = 293 °C = 293 + 273 = 566 K
Solution:
Solving equation 1 for V₂,
V₂ = V₁ × T₂ ÷ T₁
Putting values,
V₂ = (30 cm³ × 566 K) ÷ 283 K
V₂ = 60 cm³
Answer:
The solubility of the gaseous solute decreases
Explanation:
As we know, pressure decreases with altitude. This means that, at higher altitudes, the pressure is much lower than it is at sea level.
The solubility of a gas increases with increase in pressure and decreases with decrease in pressure.
Hence, in Denver, Colorado where the elevation is about 5,280 feet above sea level, a gaseous solute is less soluble than it is at sea level due to the lower pressure at such high altitude.
Answer:
O H3PO4
Explanation:
google because i looked it up
