If a sample of pure silver (Ag) contains 3.35 x 10^22 atoms of iodine, how many moles of silver are in the sample?

a. 17.9 mol

b. 2.82 mol

c. 0.180 mol

d. 0.0556 mol

Question

If a sample of pure silver (Ag) contains 3.35 x 10^22 atoms of iodine, how many moles of silver are in the sample? 

a. 17.9 mol

b. 2.82 mol

c. 0.180 mol

d. 0.0556 mol

anonymous · Answer

$$\frac{3.35x10^{22}}{6.022x10^{23}}=$$

lgbasallote · Answer

if you'd like to see the dimension analysis itself...

$$\large 3.35 \times 10^{22} \cancel{\text{atoms of iodine}} \; \times \; \frac{1 \text{mole of iodine}}{6.022 \times 10^{23} \cancel{\text{atoms of iodine}}}$$

lgbasallote · Answer

change that 1 mole of iodine into 1 mole of silver

anonymous · Answer

D 00556

anonymous · Answer

boo