calculate the average atomic mass of carbon if 98.90% of the atoms are c - 12 (12.000000 amu) and 1.100% are…

calculate the average atomic mass of carbon if 98.90% of the atoms are c - 12 (12.000000 amu) and 1.100% are c - 13 atoms (13.003354 amu). type in your answer using 2 decimal places. m_a for carbon = amu done

calculate the average atomic mass of carbon if 98.90% of the atoms are c - 12 (12.000000 amu) and 1.100% are c - 13 atoms (13.003354 amu). type in your answer using 2 decimal places. m_a for carbon = amu done

Answer

Explanation:

Step1: Convert percentages to decimals

$98.90% = 0.9890$, $1.100%=0.0110$

Step2: Use the average - atomic - mass formula

The formula for average atomic mass $M_A=\sum_{i} (x_i\times M_i)$, where $x_i$ is the abundance of isotope $i$ and $M_i$ is the mass of isotope $i$. For carbon, $M_A=(0.9890\times12.000000)+(0.0110\times13.003354)$ First term: $0.9890\times12.000000 = 11.868$ Second term: $0.0110\times13.003354=0.143036894$

Step3: Sum the results

$M_A=11.868 + 0.143036894=12.011036894\approx12.01$

Answer:

$12.01$