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Magnesium has three naturally occurring isotopes, two of which are Mg-24 (23.99 amu, 78.99%) and Mg-25...
4. (5 points) There are three major naturally occurring isotopes of magnesium, Mg-24, Mg-25 and Mg-26. The masses and percent natural abundances for Mg-24 and Mg-25 are 23.985042 amu, 78.99%; 24.985837 amu, 10.00% respectively. What must be the mass and percent natural abundance of Mg-26?
An unknown element (Element X) has three naturally occurring isotopes. Complete the table by filling in the missing percent abundance (2 decimal places). Then calculate the atomic mass of element X (1 decimal place) and determine its identity by filling in its atomic symbol (case sensitive). Isotope Abundance (%) Atomic Mass (amu) 23.985042 1 78.99 2 24.985837 10.00 3 25.982593 amu Atomic mass of element X (1 decimal place): Atomic symbol of element X:
The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is _ _amu. Isotope Abundance (%) Mass (amu) 221X 74.22 220.90 12.78 220.00 2187 13.00 218.10 2207 219.70 220.34 220.43 219.00 33.333
There are two naturally occurring isotopes of copper. 63Cu has a mass of 62.9296 amu. 65Cu has a mass of 64.9278 amu. Determine the abundance of each isotope. Number 63 0 Number 65 0
An element has two naturally-occurring isotopes. The mass numbers of these isotopes are 111 amu and 113 amu, with natural abundances of 75% and 25%, respectively. Calculate its average atomic mass.
8. An element has two naturally occurring isotopes. Isotope 1 has a mass of 120.9038 amu and a relative abundance of 57.4%. Isotope 2 has a mass of 122.9042 amu. Find the atomic mass of this element and, by comparison to the periodic table, identify it.
There are two naturally occurring isotopes of chlorine. 35^CI has a mass of 34.9689 amu. 37^CI has a mass of 36.9659 amu. Determine the abundance of each isotope.
The element europium (Z = 63) has two naturally occurring isotopes. One of the isotopes is 151 Eu, which has a mass of 150.9198 amu and a natural abundance of 47.81%. Calculate the mass of the other isotope. (Answer. 152.9 amu)
UITGUIC Potassium has three naturally occurring isotopes. They are "K (93.26%, ? amu), "K (0.0117%, 39.964 amu), and 4K (6.73%, 40.962 amu) Calculate the atomic mass of the potassium-39 isotope given that the weighted average of the isotopes is 39.099 amu and using the percent abundances of all the isotopes and the atomic masses of potassium- 40 and potassium-41. Express the mass to three decimal places and include the appropriate units. Submit Request Answer
1. An element has two naturally occurring isotopes. Isotope 1 has a mass of 120.9038 amu, and a relative abundance of 57.4%. Isotope 2 has a mass of 122.9042, and a relative abundance of 42.6%. Find the atomic mass of this element and identify it by name and symbol.