Given that Au-197 is the only natural isotope of gold,what is the mass of one Au atom and the mass of Avogadro's number of Au atoms,respectively?

Question

Quizplus · Accepted Answer

The mass of one Au atom is the atomic weight of Au-197, which is 196.97 amu.

The mass of Avogadro's number of Au atoms is calculated by multiplying the mass of one Au atom by Avogadro's number (6.022 x 10^23).

196.97 amu x 6.022 x 10^23 = 1.184 x 10^26 amu

To convert amu to grams, we need to use the conversion factor 1 amu = 1.66 x 10^-24 g.

1.184 x 10^26 amu x 1.66 x 10^-24 g/amu = 1.964 x 10^2 g

Therefore, the mass of Avogadro's number of Au atoms is 196.4 g, which is closest to choice A.

Given That Au-197 Is the Only Natural Isotope of Gold,what