# chem

Calculate the atomic mass of titanium. The five titanium isotopes have atomic masses and relative abundances of 45.953 amu (8.00%), 46.952 amu (7.30%), 47.948 amu (73.80%), 48.948 amu (5.50%), and 49.945 amu (5.40%)

1. 👍 0
2. 👎 0
3. 👁 856
1. (amu x fraction) + (amu x fraction) + (amu x fraction) + amu x fraction) + (amu x fraction).
Substitute each isotope and fraction abundance; e.g. (45.953*0.08) + (46.952*0.0730) etc etc etc = atomic mass.

1. 👍 0
2. 👎 0
2. 124.71

1. 👍 0
2. 👎 5
3. 47.867 amu

1. 👍 1
2. 👎 0
4. 47.87

(47.89 with sig figs)

1. 👍 0
2. 👎 0

## Similar Questions

1. ### chemistry

Copper used in electric wires comes in two flavors (isotopes): 63Cu and 65Cu. 63Cu has an atomic mass of 62.9298 amu and an abundance of 69.09%. The other isotope, 65Cu, has an abundance of 30.91%. The average atomic mass between

2. ### College Chemistry (Hard)

The easiest fusion reaction to initiate is 1-1H + 1-1H------> 4-2He + 1-0 n The 1-1 indicates a small one above the other on the left side of the symbol of the element.So for 1-0n is a one above a zero on the left side of n

3. ### chemistry

iridium has two isotopes. with mass numbers 191 and 193, and its average relative atomic mass is 192.23.calculate the relative abundances of the two isotopes

4. ### chemistry

The element rhenium (Re) has two naturally occurring isotopes, 185Re and 187Re, with an average atomic mass of 186.207 amu. Rhenium is 62.60% 187Re, and the atomic mass of 187Re is 186.956 amu. Calculate the mass of 185Re. am i

1. ### Chemistry

Zinc has three major and two minor isotopes. For this problem, assume that the only isotopes of zinc are the major ones, zinc-64, zinc-66, and zinc-68. The atomic mass of zinc-64 is 63.9291 Da, that of zinc-66 is 65.9260 Da, and

2. ### Chemistry

Which of the following are key parts of Dalton's Atomic Theory (Click the 4 that apply)? (1 point) All elements are composed of tiny indivisible particles called atoms*** Atoms of the same element are identical. The atoms of any

3. ### Chemistry

Boron has only two naturally occurring isotopes. The mass of boron-10 is 10.01294 amu and the mass of boron-11 is 11.00931 amu. Use the atomic mass of boron to calculate the relative abundance of boron-10. Atomic mass of boron is

4. ### physics

The atomic mass of an element is the weighted average of all of its isotopes. The percent abundance for the element boron is 19.9% boron-10 and 80.1% boron-11. Given the following atomic masses, determine the average atomic mass

1. ### Organic Chemsitry

By knowing the natural abundance of minor isotopes, it's possible to calculate the relative heights of M+ and M+1 peaks. If natural abundances are 12C - 98.9% and 13C - 1.10%, what are the relative heights, to the nearest 0.1%, of

2. ### Chemistry

There are three naturally occurring isotopes of the hypothetical element hilarium 41Hi, 42Hi, and 44Hi. The percentages of these isotopes are the following: Hilarium Natural Isotopes Abundance 41Hi 18.7% 42Hi 43.6% 44Hi 37.7% You

3. ### Chemistry

1. A hypothetical pure element consists entirely of two isotopes. The natural percent abundance of the isotope with mass 25.5 u is 86.1%. The other isotope has mass 29.2 u. Calculate the atomic weight of the naturally occurring

4. ### Chemistry

On another planet, the isotopes of titanium have the following natural abundances. Isotope 46Ti Abundance 70.900% Mass(amu) 45.95263 Isotope 48Ti Abundance 10.000% Mass(amu) 47.94795 Isotope 50Ti Abundance 19.100% Mass(amu)