an element has the following natural abundances and isotopic masses: 69.2% abundance with 62.93 amu, and…

an element has the following natural abundances and isotopic masses: 69.2% abundance with 62.93 amu, and 30.8% abundance with 64.93 amu. calculate the average atomic mass of this element. (if you wish, you can show math work for possible partial credit.)

an element has the following natural abundances and isotopic masses: 69.2% abundance with 62.93 amu, and 30.8% abundance with 64.93 amu. calculate the average atomic mass of this element. (if you wish, you can show math work for possible partial credit.)

Answer

Explanation:

Step1: Convert percentages to decimals

$69.2% = 0.692$, $30.8%=0.308$

Step2: Calculate weighted - sum

The formula for average atomic mass $A$ is $A = m_1\times x_1 + m_2\times x_2$, where $m_1$ and $m_2$ are isotopic masses and $x_1$ and $x_2$ are their respective abundances. $A=(62.93\times0.692)+(64.93\times0.308)$ $A = 62.93\times0.692=43.54756$ $A_2=64.93\times0.308 = 19.99844$ $A=43.54756 + 19.99844=63.546$

Answer:

$63.55$ amu (rounded to two decimal places)