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dalvyx [7]
3 years ago
14

The "normal" lead content in human blood is about 0.40 part per million (i.e., 0.40 g of lead per million grams of blood). A val

ue of 0.80 part per million (ppm) is considered to be dangerous. How many grams of lead are contained in 6.0 x 10^3 g of blood (the amount in an average adult) if the lead content is 0.62 ppm?
Chemistry
2 answers:
Reil [10]3 years ago
7 0

Answer:

in 6.0 E3 g of blood at a concentration of 0.62 ppm there are  3.5g of lead content

Explanation:

  • blood density: 1.06 g/L
  • ppm ≡ mg Pb / L blood

⇒ V blood = 6.0E3gblood * L / 1.06gblood = 5660.37 L blood

<u> mass of lead:</u>

⇒ 5660.37 L blood * 0.62 mg Pb / L blood * 0.001 g / mg

⇒ mass = 3.509 g of lead

djyliett [7]3 years ago
7 0

Answer:

3.7 × 10⁻³ g Pb

Explanation:

0.62 parts per million means that there are 0.62 g of lead per million grams of blood (10⁶ grams of blood). In order to find the grams of lead on 6.0 × 10³ grams of blood (the amount in an average adult), we will use a conversion fraction.

6.0 × 10³ g blood × (0.62 g Pb/ 10⁶ g blood) = 3.7 × 10⁻³ g Pb

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<span><span>m1</span><span>(<span>Tf</span>l–l<span>T<span>∘1</span></span>)</span>+<span>m2</span><span>(<span>Tf</span>l–l<span>T<span>∘2</span></span>)</span>=0</span>

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8 0
3 years ago
Which of the following statements are correct regarding the binding energy?
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None of the above?
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8 0
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3 0
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What role does valence electrons play in reactivity for an element?
kirza4 [7]

Explanation:

The valence electrons within an atom is the number of electrons in its outermost shell.

These electrons are used by an atom to react with one another. They  determine the extent to which an atom is ready to combine either by losing, gaining or sharing these electrons.

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4 0
3 years ago
a water sample is found to have a cl- content of 100ppm as nacl what is the concentration of chloride in moles per liter
ladessa [460]

Answer:

The concentration of chloride ion is 2.82\times10^{-3}\;mol/L

Explanation:

We know that 1 ppm is equal to 1 mg/L.

So, the Cl^- content 100 ppm suggests the presence of 100 mg of Cl^- in 1 L of solution.

The molar mass of Cl^- is equal to the molar mass of Cl atom as the mass of the excess electron in Cl^- is negligible as compared to the mass of Cl atom.

So, the molar mass of Cl^- is 35.453 g/mol.

Number of moles = (Mass)/(Molar mass)

Hence, the number of moles (N) of Cl^- present in 100 mg (0.100 g) of Cl^- is calculated as shown below:

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So, there is 2.82\times10^{-3}\;mol of Cl^- present in 1 L of solution.

5 0
3 years ago
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