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Irina-Kira [14]
3 years ago
9

A 171 g sample of tetrafluoromethane (CF4) contains 90 g of carbon. What is the mass percent of fluorine in the compound?

Chemistry
2 answers:
inn [45]3 years ago
8 0
<span>To find the mass percent of fluorine in the compound, you must first determine the mass in g of fluorine in the compound. We do this by subtracting the mass of carbon from the total mass of the sample. From this we get 171 - 90 = 81g of fluorine in CF4 sample. Now to get the mass percent, we divide the fluorine mass by the sample mass to get the percent mass. 81/171 = .4737 which multiplied by 100 to get percentage give 47.37%.</span>
rodikova [14]3 years ago
8 0
<span>Mass of fluorine:171 g (compound ) - 90 ( carbon )  =>  81 g of

fluorinepercent of fluorine in the compound:

( 81 g F ) / 171 ( compound ) x  100 %

= 0,4737 x 100 = 47,37%

hope this helps!</span>
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Find the mass in grams of 3.00 x 1023 molecules of F2
LUCKY_DIMON [66]
<h3>Answer:</h3>

18.9 g F₂

<h3>General Formulas and Concepts:</h3>

<u>Math</u>

<u>Pre-Algebra</u>

Order of Operations: BPEMDAS

  1. Brackets
  2. Parenthesis
  3. Exponents
  4. Multiplication
  5. Division
  6. Addition
  7. Subtraction
  • Left to Right

<u>Chemistry</u>

<u>Atomic Structure</u>

  • Reading a Periodic Table
  • Using Dimensional Analysis
  • Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.
<h3>Explanation:</h3>

<u>Step 1: Define</u>

3.00 × 10²³ molecules F₂

<u>Step 2: Identify Conversions</u>

Avogadro's Number

Molar Mass of F₂ (Diatomic) - 38.00 g/mol

<u>Step 3: Convert</u>

  1. Set up:                              \displaystyle 3.00 \cdot 10^{23} \ molecules \ F_2(\frac{1 \ mol \ F_2}{6.022 \cdot 10^{23} \ molecules \ F_2})(\frac{38.00 \ g \ F_2}{1 \ mol F_2})
  2. Multiply:                                                                                                             \displaystyle 18.9306 \ g \ F_2

<u>Step 4: Check</u>

<em>Follow sig fig rules and round. We are given 3 sig figs.</em>

18.9306 g F₂ ≈ 18.9 g F₂

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