Hamaranayy
Answered

  1. A sample of gold (Au) has a mass of 35.12 g.
ACalculate the number of moles of gold (Au) in the sample and record in

Table 1. Show your work.

BCalculate the number of atoms of gold (Au) in the sample and record

in Table 1. Show your work.

  1. A sample of table sugar (sucrose, C12H22O11) has a mass of 1.202 g.
ACalculate the number of moles of C12H22O11 contained in the sample

and record in Table 1. Show your work.

Verified Answer :

o solve this, first convert the sample into moles. 

35.12g Au (1mol/197g) = 0.18 mol Au 

Then, using this mole value, convert into atoms by multiplying by Avogadro's number: 

0.18 mol (6.022 10^23 atoms/1 mol) = 1.0810^23 atom

2. Again, start by converting to moles using the molar mass: 

12 mol C = 1212 = 144g 
22 mol H = 221 = 22g 
11 mol O = 1116 = 176 g 
---------------------------------------... 
C12H22011 = 144+22+176 = 342g/mol 

Then use that value to convert the mass to moles. 
2
1.202g C12H22O11 (1mol / 342g) = 3.510^-3 mol C12H22O11 


b. 3.510^-3 (144/342) = 1.510^-3mol C 
etc.
 follow the same procedure as b, but with atom value

Related Questions