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

Answer:

There is $12277.494g$ of CO2

Explanation:

We know that the molar mass of CO2 is $44.01\frac{g}{mol}$

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 :

$x=\frac{(44.01).(1.68).10^{26}}{(6.02214076).10^{23}}g=12277.494g$

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