Question

There are three naturally occurring isotopes of the hypothetical element hilarium 45Hi, 46Hi, and 48Hi. The percentages of these isotopes are the following: Hilarium Natural Isotopes Abundance 45Hi 18.3% 46Hi 34.5% 48Hi 47.2% You can assume that the atomic masses are exactly equal to the mass number. Calculate the weight of "naturally" occurring hilarium and report it as you would for any other naturally occurring element. Answer in units of g/mol. Your answer must be within ± 0.005%

Answer 1

The weighted average atomic mass of naturally occurring hilarium is approximately 46.761 g/mol.

Step-by-step explanation:

To calculate the average atomic mass of hilarium, we need to multiply the abundance of each isotope by its mass, and then sum the results.

For hilarium-45 (18.3% abundance), the mass would be (0.183 * 45) = 8.235 g/mol.

For hilarium-46 (34.5% abundance), the mass would be (0.345 * 46) = 15.87 g/mol.

For hilarium-48 (47.2% abundance), the mass would be (0.472 * 48) = 22.656 g/mol.

Adding up these three masses, we get (8.235 + 15.87 + 22.656) = 46.761 g/mol.

Therefore, the weighted average atomic mass of naturally occurring hilarium is approximately 46.761 g/mol.