Answer:
Explanation:
Hello there!
In this case, according to the given information, it turns out possible for us to find the molecular formula of the given compound by firstly calculating both moles and grams of carbon in carbon dioxide and hydrogen in water, as the only sources of these elements derived from the compound x due to its combustion:
Now, since the addition of carbon and hydrogen is about 6.50 grams, we infer the compound has no oxygen, that is why we now set the mole ratios in the empirical formula for both C and H as shown below:
Yet it cannot be decimal, that is why we multiply by 4 to get the correct whole-numbered empirical formula:
Whose molar mass is 64.09 g/mol, which makes the ratio of molar masses:
Therefore, the molecular formula is twice the empirical one:
Regards!
20 cups of flour, 30 eggs, and 10 cups of sugar
<h3>
Answer:</h3>
121 mol 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>Organic</u>
- Writing chemical compounds
- Writing organic structures
- Prefixes
- Alkanes, Alkenes, Alkynes
<u>Atomic Structure</u>
- Using Dimensional Analysis
- Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.
<h3>
Explanation:</h3>
<u>Step 1: Define</u>
7.31 × 10²⁵ molecules CH₄
<u>Step 2: Identify Conversions</u>
Avogadro's Number
<u>Step 3: Convert</u>
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<u />
<u>Step 4: Check</u>
<em>Follow sig fig rules and round. We are given 3 sig figs.</em>
121.388 mol CH₄ ≈ 121 mol CH₄
Answer:
All of the above
Explanation:
Their all chemical change
One lead atom, two nitrogen atoms, four oxygen atoms.
