nitrogen has two isotopes. one has an atomic mass of 14.003 amu and a relative abundance of 99.63% while the…

nitrogen has two isotopes. one has an atomic mass of 14.003 amu and a relative abundance of 99.63% while the other isotope has an atomic mass of 15.000 amu and a relative abundance of 0.37%. what is the average atomic mass for nitrogen?\na 14.007 amu\nb 14.778 amu\nc 14.456 amu\nd 14.993 amu

nitrogen has two isotopes. one has an atomic mass of 14.003 amu and a relative abundance of 99.63% while the other isotope has an atomic mass of 15.000 amu and a relative abundance of 0.37%. what is the average atomic mass for nitrogen?\na 14.007 amu\nb 14.778 amu\nc 14.456 amu\nd 14.993 amu

Answer

Explanation:

Step1: Convert percentages to decimals

$99.63% = 0.9963$, $0.37%=0.0037$

Step2: Calculate weighted - sum

The formula for average atomic mass is $\sum_{i} (m_i\times a_i)$, where $m_i$ is the atomic mass of the isotope and $a_i$ is its relative abundance. So, $(14.003\times0.9963)+(15.000\times0.0037)$ $=14.003\times0.9963 + 15\times0.0037$ $=13.9411989+0.0555$ $=14.007$ amu

Answer:

A. 14.007 amu