How many grams are in 1.76 x 10^23 atoms of iodine

Explanation:

To convert from atoms to grams, you must first convert atoms to moles, then moles to grams.

1. Convert Atoms to Moles

To convert atoms to grams, Avogadro's number must be used.

This number tells us the number of particles (atoms, molecules, ions, etc.) in 1 mole. In this case, the particles are atoms of iodine.

Multiply the given number of atoms by Avogadro's number.

Flip the fraction so the atoms of iodine will cancel out.

Multiply so the problem condenses into 1 fraction.

2. Convert Moles to Grams

Now we must use the molar mass of iodine, which is found on the Periodic Table.

Use this mass as a fraction.

Multiply this fraction by the number of moles found above.

Multiply. The moles of iodine will cancel.

The 1 as a denominator is insignificant.

3. Round

The original measurement of 1.76*10^23 has 3 significant figures (1, 7, and 6). Therefore we must round our answer to 3 sig figs. For this answer, that is the tenths place.

The 8 in the hundredth place tells us to round the 0 up to a 1.

There is about 37.1 grams of iodine in 1.76*10^23 atoms.

*tilts head* sounds more like a statement

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: