An element has two naturally occurring isotopes with atomic masses of 112.90 amu and 114.90 amu. the relative abundances of these isotopes are 4.29% and 95.71%, respectively. what is the average atomic mass of the element? a.22.78 amu b.113.9 amu c.114.8 amu d.227.8 amu

C. 114.8 u

Explanation:

The atomic mass of X is the weighted average of the atomic masses of its isotopes.

We multiply the atomic mass of each isotope by a number representing its relative importance (i.e., its percent of the total).

Set up a table for easy calculation

0.0429 × 112.90 u =     4.843 u

0.9571  × 114.90 u = 109.97    u

                 TOTAL = 114.8       u

not clear

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.