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To determine the mass of nickel in a 2,400 gram sample of propanol where the concentration of nickel is 20 ppb (parts per billion), let us break down the steps:
1. Understand the concentration in ppb:
- ppm (parts per million) means 1 unit of substance per 1,000,000 units of the medium.
- Similarly, ppb (parts per billion) means 1 unit of substance per 1,000,000,000 units of the medium.
2. Convert the concentration from ppb to a fractional form:
- 20 ppb can be represented as [tex]\( \frac{20}{1,000,000,000} \)[/tex].
3. Calculate the mass of nickel:
- We know the sample mass is 2,400 grams.
- Therefore, the mass of nickel in the sample is calculated by multiplying the sample mass by the concentration fraction:
[tex]\[ \text{Mass of Nickel} = \text{Sample Mass} \times \frac{\text{Concentration (ppb)}}{1,000,000,000} \][/tex]
4. Perform the multiplication:
- [tex]\(\text{Mass of Nickel} = 2,400 \, \text{g} \times \frac{20}{1,000,000,000}\)[/tex]
[tex]\[ \text{Mass of Nickel} = 2,400 \times 20 \times 10^{-9} \, \text{g} \][/tex]
[tex]\[ \text{Mass of Nickel} = 48,000 \times 10^{-9} \, \text{g} \][/tex]
5. Simplified result:
- Simplify [tex]\(48,000\)[/tex] times [tex]\(10^{-9}\)[/tex]:
[tex]\[ 48,000 \times 10^{-9} = 4.8 \times 10^{-5} \, \text{g} \][/tex]
Thus, the mass of nickel in the 2,400 gram sample of propanol is [tex]\(4.8 \times 10^{-5} \, \text{g}\)[/tex].
Comparing this result to the given options:
A. [tex]\(0.0083 \, \text{g Ni}\)[/tex]
B. [tex]\(4.8 \times 10^3 \, \text{g Ni}\)[/tex]
C. [tex]\(8.3 \times 10^0 \, \text{g Ni}\)[/tex]
D. [tex]\(0.048 \, \text{g Ni}\)[/tex]
None of these options exactly match our calculated result. Therefore, the question or answer choices might contain an error and should be reviewed for possible correction.
1. Understand the concentration in ppb:
- ppm (parts per million) means 1 unit of substance per 1,000,000 units of the medium.
- Similarly, ppb (parts per billion) means 1 unit of substance per 1,000,000,000 units of the medium.
2. Convert the concentration from ppb to a fractional form:
- 20 ppb can be represented as [tex]\( \frac{20}{1,000,000,000} \)[/tex].
3. Calculate the mass of nickel:
- We know the sample mass is 2,400 grams.
- Therefore, the mass of nickel in the sample is calculated by multiplying the sample mass by the concentration fraction:
[tex]\[ \text{Mass of Nickel} = \text{Sample Mass} \times \frac{\text{Concentration (ppb)}}{1,000,000,000} \][/tex]
4. Perform the multiplication:
- [tex]\(\text{Mass of Nickel} = 2,400 \, \text{g} \times \frac{20}{1,000,000,000}\)[/tex]
[tex]\[ \text{Mass of Nickel} = 2,400 \times 20 \times 10^{-9} \, \text{g} \][/tex]
[tex]\[ \text{Mass of Nickel} = 48,000 \times 10^{-9} \, \text{g} \][/tex]
5. Simplified result:
- Simplify [tex]\(48,000\)[/tex] times [tex]\(10^{-9}\)[/tex]:
[tex]\[ 48,000 \times 10^{-9} = 4.8 \times 10^{-5} \, \text{g} \][/tex]
Thus, the mass of nickel in the 2,400 gram sample of propanol is [tex]\(4.8 \times 10^{-5} \, \text{g}\)[/tex].
Comparing this result to the given options:
A. [tex]\(0.0083 \, \text{g Ni}\)[/tex]
B. [tex]\(4.8 \times 10^3 \, \text{g Ni}\)[/tex]
C. [tex]\(8.3 \times 10^0 \, \text{g Ni}\)[/tex]
D. [tex]\(0.048 \, \text{g Ni}\)[/tex]
None of these options exactly match our calculated result. Therefore, the question or answer choices might contain an error and should be reviewed for possible correction.
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