How would the concentration of silver ions compare in a 1.0 x 10-16 L saturated solution to a 1.5 x 10-16 L saturated solution?
1 answer:
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Answer:
Explanation:
To convert from atoms to grams, you must first convert atoms to moles, then moles to grams.
1. Convert Atoms to Moles
To convert atoms to grams, Avogadro's number must be used.
This number tells us the number of particles (atoms, molecules, ions, etc.) in 1 mole. In this case, the particles are atoms of iodine.
Multiply the given number of atoms by Avogadro's number.
Flip the fraction so the atoms of iodine will cancel out.
Multiply so the problem condenses into 1 fraction.
2. Convert Moles to Grams
Now we must use the molar mass of iodine, which is found on the Periodic Table.
- Iodine Molar Mass: 126.9045 g/mol
Use this mass as a fraction.
Multiply this fraction by the number of moles found above.
Multiply. The moles of iodine will cancel.
The 1 as a denominator is insignificant.
3. Round
The original measurement of 1.76*10^23 has 3 significant figures (1, 7, and 6). Therefore we must round our answer to 3 sig figs. For this answer, that is the tenths place.
The 8 in the hundredth place tells us to round the 0 up to a 1.
There is about <u>37.1 grams of iodine </u>in 1.76*10^23 atoms.
Answer: m = 11.2 g C7H16
Explanation: First convert the mass of CO2 to moles. Then do the mole ratio between CO2 and C7H16 which is 7:1. Finally convert the moles of C7H16 to the mass of C7H16.
Solution attached.
