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Svetradugi [14.3K]
3 years ago
11

The radius of a uranium atom is 149 pm. How many uranium atoms would have to be laid side by side to span a distance of 4.96 mm?

Chemistry
2 answers:
nikitadnepr [17]3 years ago
4 0

Answer:

4960000000 pm

Explanation:

4.96*1000000000= 4960000000

djverab [1.8K]3 years ago
3 0

Answer:

Uranium atoms required to be laid side by side to span a distance of 4.96 mm is 1.6644\times 10^7 atoms.

Explanation:

The radius of a uranium atom ,r = 149 pm =1.49\times 10^{-7} mm

1 pm=10^{-9} mm

The diameter of a uranium atom ,d =

d = 2r =2\times 1.49\times 10^{-7} mm=2.98\times 10^{-7} mm

The let the uranium atom to be laid side by side to span a distance of 4.96 mm be x.

x\times d=4.96 mm

x=\frac{4.96 mm}{d}=\frac{4.96 mm}{2.98\times 10^{-7} mm}=1.6644\times 10^7 atoms.

Uranium atoms required to be laid side by side to span a distance of 4.96 mm is 1.6644\times 10^7 atoms.

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Answer:

a. 0.180M of C₆H₅NH₂

b. 0.0887M C₆H₅NH₃⁺

c. pH = 2.83

Explanation:

a. Based in the chemical equation:

C₆H₅NH₂(aq) + HCl(aq) → C₆H₅NH₃⁺(aq) + Cl⁻(aq)

<em>1 mole of aniline reacts per mole of HCl</em>

Moles required to reach equivalence point are:

Moles HCl = 0.02567L ₓ (0.175mol / L) = 4.492x10⁻³ moles HCl = moles C₆H₅NH₂

As the original solution had a volume of 25.0mL = 0.0250L:

4.492x10⁻³ moles C₆H₅NH₂ / 0.0250L = 0.180M of C₆H₅NH₂

b. At equivalence point, moles of C₆H₅NH₃⁺ are equal to initial moles of C₆H₅NH₂, that is 4.492x10⁻³ moles

But now, volume is 25.0mL + 25.67mL = 50.67mL = 0.05067L. Thus, molar concentration of C₆H₅NH₃⁺ is:

[C₆H₅NH₃⁺] = 4.492x10⁻³ moles / 0.05067L = 0.0887M C₆H₅NH₃⁺

c. At equivalence point you have just 0.0887M C₆H₅NH₃⁺ in solution. C₆H₅NH₃⁺ has as equilibrium in water:

C₆H₅NH₃⁺(aq) + H₂O(l) → C₆H₅NH₂ + H₃O⁺

Where Ka = Kw / Kb = 1x10⁻¹⁴ / 4.0x10⁻¹⁰ =

<em>2.5x10⁻⁵ = [C₆H₅NH₂] [H₃O⁺] / [C₆H₅NH₃⁺]</em>

When the system reaches equilibrium, molar concentrations are:

[C₆H₅NH₃⁺] = 0.0887M - X

[C₆H₅NH₂] = X

[H₃O⁺] = X

Replacing in Ka formula:

2.5x10⁻⁵ = [X] [X] / [0.0887M - X]

2.2175x10⁻⁶ - 2.5x10⁻⁵X = X²

0 = X² + 2.5x10⁻⁵X - 2.2175x10⁻⁶

Solving for X:

X = -0.0015 → False solution. There is no negative concentrations.

X = 0.001477 → Right solution.

As [H₃O⁺] = X, [H₃O⁺] = 0.001477

Knowing pH = -log [H₃O⁺]

pH = -log 0.001477

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