Question

how many moles of co2 will left if 10^21 molecules are removed from 513.07mg of co2

Answer 1

Answer:-

0.01 mole

Explanation:-

• Molar mass of Carbon (C) = 12g/mol

• Molar mass of Oxygen (O) = 16g/mol

• Avogadro Number = 6.022×10²³

Hence, molar mass of CO₂ :-

= 12 + 16×2

= 12 + 32

= 44g/mol

• Given Mass of CO₂ :-

= 513.07mg= 0.51307g

Number of moles in 0.51307g of CO₂ :-

= Given Mass/Molar mass

= 0.51307/44

= 0.0116 mole [approximately]

Now, from 0.116 moles of CO₂ , 10²¹ molecules are removed.

Number of moles in 10²¹ molecules

of CO₂ :-

= No of molecules/Avogadro Number

= 10²¹/[6.022×10²³]

= 1/[6.022×10²]

= 1/602.2

= 0.0016 mole [approximately]

Therefore, number of moles of CO₂ left :-

= 0.0116 - 0.0016

= 0.01 mole

Thus, 0.01 mole of CO₂ are left.

Answer 2

To find:

How many moles of co2 will left if 10²¹ molecules are removed from 513.07mg of CO2.

Calculation:

Moles of CO2 (carbon dioxide) in 513.07 mg :

$\rm \therefore \: no. \: of \: moles = \dfrac{given \: mass}{molar \: mass}$

$\rm \implies \: no. \: of \: moles = \dfrac{0.513}{44}$

$\rm \implies \: no. \: of \: moles = 0.0116$

Now, number of moles associated with 10²¹ molecules of CO2 :

$\rm \therefore \: no. \: of \: moles = \dfrac{no. \: of \: molecules}{avagadro \: no.}$

$\rm \implies\: no. \: of \: moles = \dfrac{ {10}^{21} }{6.023 \times {10}^{23} }$

$\rm \implies\: no. \: of \: moles = 0.167 \times {10}^{ - 2}$

$\rm \implies\: no. \: of \: moles = 0.0016$

So, number of moles left :

$\rm moles \: left = 0.0116 - 0.0016$

$\implies\rm moles \: left = 0.01$

So, number of moles left is 0.01