Answer:
false
Explanation:
the magnetic domains in the area around a magnet where the force acts.
<span>Converting from mass (grams) to moles: Divide your initial mass by the molar mass of the compound as determined by the periodic table.<span>Converting from moles to mass (grams): </span>Multiply your initial mole value by the molar mass of the compound as determined by the periodic table.<span>Converting from volume (liters) to moles: </span>Divide your initial volume by the molar volume constant, 22.4 L.<span>Converting from moles to volume (liters): </span>Multiply your mole value by the molar volume constant, 22.4L.<span>Converting from particles (atoms, molecules, or formula units) to moles: </span>Divide your particle value by Avogadro’s number, 6.02×1023. Remember to use parentheses on your calculator!<span>Converting from moles to particles (atoms, molecules, or formula units): </span>Multiply your mole value by Avogadro’s number, 6.02×1023.<span>Mole-to-mole conversions: </span>Use the coefficients from your balanced equation to determine your conversion factor. Be sure your units cancel out so you end up with the correct mole value.</span>
Before you begin titration, drops of indicator are added to the Erlenmeyer flask. This happens when preparing to measure pH change.
<u>Answer:</u> The average atomic mass of element X is 59.3 amu.
<u>Explanation:</u>
Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.
Formula used to calculate average atomic mass follows:
.....(1)
- <u>For isotope 1 (X-59) :</u>
Mass of isotope 1 = 59.015 amu
Percentage abundance of isotope 1 = 91.7 %
Fractional abundance of isotope 1 = 0.917
- <u>For isotope 2 (X-62) :</u>
Mass of isotope 2 = 62.011 amu
Percentage abundance of isotope 2 = (100 - 91.7) % = 8.3 %
Fractional abundance of isotope 2 = 0.083
Putting values in equation 1, we get:
![\text{Average atomic mass of X}=[(59.015\times 0.917)+(62.011\times 0.083)]](https://tex.z-dn.net/?f=%5Ctext%7BAverage%20atomic%20mass%20of%20X%7D%3D%5B%2859.015%5Ctimes%200.917%29%2B%2862.011%5Ctimes%200.083%29%5D)
Hence, the average atomic mass of element X is 59.3 amu.
