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Dima020 [189]
3 years ago
11

Consider a hypothetical element x that consists of two isotopes, one with a mass of 41.99998 amu and the other with a mass of 44

.99987 amu. their percent abundances are 33.3333% and 66.6667%, respectively. without doing an actual calculation, the mass closest to the atomic mass of x is
Chemistry
1 answer:
Dafna11 [192]3 years ago
4 0
To determine the average atomic weight of the hypothetical element X, you essentially take the average of the isotopes based on the percent abundance of each isotope present.

However, to do this "without doing an actual calculation" is not possible. But we can do it with very simplified calculations. We have one isoptope of X that is 42 amu that is 1/3 of the element, and the other isotope which is 45 amu that is 2/3 of the element.

A simple calculation to find the mass of X is as follows:

(1/3)(42 amu) + (2/3)(45 amu) = atomic weight of X.
14 + 30 = atomic weight of X
Atomic weight of X = 44 amu.

The mass closest to the atomic mass of X is 44 amu.
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About 55L of a gas in a flexible container is under a pressure of 3.2 atm and at a temperature of 520K. What is the new volume o
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Answer:

30.62 L

Explanation:

From the question given above, the following data were obtained:

Initial volume (V₁) = 55 L

Initial pressure (P₁) = 3.2 atm

Initial temperature (T₁) = 520 K

Final temperature (T₂) = 760 K

Final pressure (P₂) = 8.4 atm

Final volume (V₂) =?

The final volume of the gas can be obtained as follow:

P₁V₁ / T₁ = P₂V₂ / T₂

3.2 × 55 / 520 = 8.4 × V₂ / 760

176 / 520 = 8.4 × V₂ / 760

Cross multiply

520 × 8.4 × V₂ = 176 × 760

4368 × V₂ = 133760

Divide both side by 4368

V₂ = 133760 / 4368

V₂ = 30.62 L

Therefore, the new volume of the gas is 30.62 L

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A 25. 0-ml sample of 0. 150 m hydrocyanic acid is titrated with a 0. 150 m naoh solution. What is the ph beforeany base is added
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How many formula units are there in 50.3 moles potassium chloride?
Alona [7]
<h3>Answer:</h3>

3.03 × 10²⁵ formula units KCl

<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>Unit 0</u>

  • Reading a Periodic Table
  • Writing Compounds

<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>

50.3 mol KCl (Potassium chloride)

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

Avogadro's Number

<u>Step 3: Convert</u>

<u />\displaystyle 50.3 \ mol \ KCl(\frac{6.022 \cdot 10^{23} \ formula \ units \ KCl}{1 \ mol \ KCl} ) = 3.02907 × 10²⁵ formula units KCl

<u>Step 4: Check</u>

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

3.02907 × 10²⁵ formula units KCl ≈ 3.03 × 10²⁵ formula units KCl

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