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Leni [432]
3 years ago
8

How many moles of aluminum are equivalent to 4.816x10^24 atoms? 12.5 8 1.25 0.8

Chemistry
2 answers:
krek1111 [17]3 years ago
6 0

Answer:

Eight

Explanation:

kotegsom [21]3 years ago
4 0

Answer:

8

Explanation:

1 mole = 6.02 × 10²³ atoms

? moles = 4.816 × 10²⁴ atoms.

? Moles = 4.816 × 10²⁴ ÷ 6.02 × 10²³

? Moles = 8 moles

8 moles of aluminum = 4.816 × 10²⁴

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Tree sap flows over the leaf and preserves it.

Explanation:

Amber would preserve the image.

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Which statement about the organisms whose fossils are found in the rock is correct?
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a?

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Explain the first three steps of scientific inquiry
erastovalidia [21]
1. Observation-- making observations and taking notes about what you see, smell, hear, think, etc.
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5 0
3 years ago
How many moles are in 1.51x10^26 atoms of xenon (Xe)? Please and thank you :)!!
RoseWind [281]
<h3>Answer:</h3>

251 mol Xe

<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>

  • Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.

<u>Stoichiometry</u>

  • Using Dimensional Analysis
<h3>Explanation:</h3>

<u>Step 1: Define</u>

[Given] 1.51 × 10²⁶ atoms Xe

[Solve] moles Xe

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

Avogadro's Number

<u>Step 3: Convert</u>

  1. [DA] Set up:                                                                                                     \displaystyle 1.51 \cdot 10^{26} \ atoms \ Xe(\frac{1 \ mol \ Xe}{6.022 \cdot 10^{23} \ atoms \ Xe})
  2. [DA] Multiply/Divide [Cancel out units]:                                                         \displaystyle 250.747 \ mol \ Xe

<u>Step 4: Check</u>

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

250.747 mol Xe ≈ 251 mol Xe

3 0
3 years ago
Solution A is 0.44 M and reacts with 0.11 M of solution B. Assume that the value of x is 0, the value of y is 1, and r is 1.07 ×
xz_007 [3.2K]

Answer:

K, the rate constant = 9.73 × 10^(-1)/s

Explanation:

r = K × [A]^x × [B]^y

r = Rate = 1.07 × 10^(-1)/s

K = Rate constant

A and B = Concentration in mol/dm^-3

A = 0.44M

B = 0.11M

x = Order of reaction with respect to A = 0

y = Order of reaction with respect to B = 1

Solving, we get

r/([A]^x × [B]^y) = K

K = 1.07 × 10^(-1)/s/(0.44^0 × 0.11^1)= 0.9727

K = 0.9727

7 0
3 years ago
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