Explanation:
Moles of NaOH = 10g / (40g/mol) = 0.25mol.
0.25mol / 500g = 0.50mol / 1000g = 0.50mol/dm³.
The molarity is 0.50mol/dm³.
<h3>
Answer:</h3>
25.4 g CH₄
<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>
1.58 mol CH₄
<u>Step 2: Identify Conversions</u>
[PT] Molar Mass of C - 12.01 g/mol
[PT] Molar Mass of H - 1.01 g/mol
Molar Mass of CH₄ - 12.01 + 4(1.01) = 16.05 g/mol
<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>
25.359 g CH₄ ≈ 25.4 g CH₄
C(5) + O2(g)
Hope this helped
Answer:
She could prove that it is a combination of substances by looking for a change in color, or the formation of bubbles. She could also try to pull the combination apart by physical means alone.
Explanation:
<u>Answer:</u> The equilibrium concentration of CO is 0.243 atm
<u>Explanation:</u>
We are given:
Initial partial pressure of carbon dioxide = 0.902 atm
As, carbon dioxide is present initially. This means that the reaction is proceeding backwards.
For the given chemical equation:

<u>Initial:</u> 0.902
<u>At eqllm:</u> 3x (0.902-3x)
The expression of
for above equation follows:

We are given:

Putting values in above equation, we get:

So, equilibrium concentration of CO = 3x = (3 × 0.0810) = 0.243atm[/tex]
Hence, the equilibrium concentration of CO is 0.243 atm