Lithium has two naturally occurring isotopes, 6Li (isotopic mass = 6.02 amu) and 7Li (isotopic mass = 7.02 amu). Lithium has an atomic mass of 6.94 amu. What is the percent abundance of lithium–6? 92.50% 86.66% 46.16% 8.00% 6.080%

0 On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u) 79.600% 45.95263 13.400% 47.94795 50 Ti 7.000% 49.94479 What is the average atomic mass of titanium on that planet? $ 4 R F average atomic mass= Isotope 46 Ti 48 Ti V 888 F4 % 5 T G F5 B 6 Y MacBook Air H & 7 N U F7 J * 00 8 M DII FB K ( 9 F9 H O O F10 P F11 + = 100 I F12

A cylindrical piece of pure titanium (Ti, density=4.506 g/cm^3) has diameter d=1.15 cm and length L=153 mm. How many atoms of titanium are in the cylinder? Use 47.87 g/mol for the average atomic mass of naturally occurring Ti. volume of cylinder=pie d^2L/4 Avogadro's number=6.022 x 10^23

On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u) 74.200% 45.95263 15.100% 47.94795 10.700% 49.94479 Isotope 46 Ti 48 Ti 50 Ti What is the average atomic mass of titanium on that planet? average atomic mass= x10 TOOLS u

3) Atmospheric argon is a mixture of three stable isotopes 36Ar, 38Ar, and 40Ar.  Use the information below to determine the atomic mass and natural abundance of 40Ar.  The atomic weight of argon is 39.948 u.                      Argon-36             35.967545 u                       0.337% Argon-38             37.96732 u                         0.063% Argon-40             ?                                              ?

An unknown element is a mixture of isotopes 120X and 122X. The average atomic mass of X is 121.03 amu. What is the percent abundance of 122X?

A certain element has five stable isotopes with the following masses and percent abundance: Isotope 1:   63.929147 amu,   48.63% Isotope 2:   65.926037 amu,   27.90% Isotope 3:   66.927131 amu,    4.100% Isotope 4:   67.924848 amu,   18.75% Isotope 5:   69.925325 amu,     0.6200%      What is the atomic mass of this element? (Do not round intermediate calculations.)

6) Complete the following table by calculating the atomic mass. Isotope Mass of Atom (u) Percent Abundance (%) ¹H 2H 12C 13C 160 170 180 1.007825 2.1040 12.0 13.003355 15.994915 16.999131 17.999160 99.985 0.015 98.90 1.10 99.762 0.038 0.200 Atomic Mass (u)

3) Calculate the atomic mass of the following element with three isotopes (masses and relative abundances given below). Referring to the periodic table, identify the element. 27.9769 u, 92.2232% 28.9765 u, 4.6858% 29.9738 u, 3.0921%