Question

How many grams are in 1.68 x 1026 molecules of CO2? (molar mass=44.01 g/mol) (Hint: You will need to use your entire stoichiometry flow chart)

Answer 1

According to Avogadro's law 1 mole contains 6.022 ×10^23 particles
1 mole of carbon = 44.01 g/ mol
Therefore;
44.01 g = 6.022 ×10^23 molecules
Hence, 1.68×10^26 molecules will have a mass of ;
(44.01 × 1.68×0^26) / 6.022×10^23
= 1.228 × 10^4 molecules

Answer 2

There is
`12277.494g` of CO2

Step-by-step explanation:

We know that the molar mass of CO2 is
`44.01(g)/(mol)`

This means that in 1 mole of molecules of CO2 is 44.01 g of CO2

In one mole of molecules of any substance there are N molecules where N is defined as the Avogadro number.

`N=AvogadroNumber=(6.02214076).10^(23)`

Therefore, we can write that

In
`(6.02214076).10^(23)` molecules of CO2 (1 mole of CO2) there is 44.01 g of CO2 ⇒

In
`(1.68).10^(26)` molecules of CO2 there will be x grams :

`x=((44.01).(1.68).10^(26))/((6.02214076).10^(23))g=12277.494g`

We answer that in
`(1.68).10^(26)` molecules of CO2 there is
`12277.494g` of CO2