Question

carbon has two naturally occurring isotopes: carbon - 12 (abundance = 98.90%, mass = 12.000 amu) and carbon - 13 (abundance = 1.10%, mass = 13.0033 amu). calculate the atomic mass of carbon. (1 point) 12.01 amu 25.00 amu 12.86 amu 12.50 amu

Explanation:

Step1: Convert abundances to decimals

Carbon - 12 abundance: \(98.90\%=0.9890\)
Carbon - 13 abundance: \(1.10\% = 0.0110\)

Step2: Calculate contribution of each isotope

Contribution of carbon - 12: \(0.9890\times12.000=11.868\)
Contribution of carbon - 13: \(0.0110\times13.0033 = 0.1430363\)

Step3: Sum the contributions

Atomic mass of carbon: \(11.868+0.1430363=12.0110363\approx12.01\)

Answer:

12.01 amu