the table below gives the atomic mass and relative abundance values for the three isotopes of element…

the table below gives the atomic mass and relative abundance values for the three isotopes of element m.\n|relative abundance (%)|atomic mass (amu)|\n|----|----|\n|78.99|23.9850|\n|10.00|24.9858|\n|11.01|25.9826|\nwhat is the average atomic mass (in amu) of element m?\no 2.86\no 5.36\no 24.30\no 24.98

the table below gives the atomic mass and relative abundance values for the three isotopes of element m.\n|relative abundance (%)|atomic mass (amu)|\n|----|----|\n|78.99|23.9850|\n|10.00|24.9858|\n|11.01|25.9826|\nwhat is the average atomic mass (in amu) of element m?\no 2.86\no 5.36\no 24.30\no 24.98

Answer

Answer:

24.30

Explanation:

Step1: Convert percentages to decimals

$78.99% = 0.7899$, $10.00%=0.1000$, $11.01% = 0.1101$

Step2: Calculate weighted - mass for each isotope

For the first isotope: $0.7899\times23.9850 = 18.9548$ For the second isotope: $0.1000\times24.9858 = 2.4986$ For the third isotope: $0.1101\times25.9826=2.8607$

Step3: Sum up the weighted - masses

$18.9548 + 2.4986+2.8607=24.3141\approx24.30$