Answer :
Answer:
The number of carbon atoms in 52.06 g of CO₂ is 7.124 x 10²³ atoms
Explanation:
The number of carbon atoms can be determined by taking the product of the Avogadro's number and the number of moles of CO₂. The moles of CO₂ can be calculated as,
[tex]n_{CO_2}=\frac{mass}{molecular mass}[/tex]
[tex]n_{CO_2}=\frac{52.06}{44.01}[/tex]
[tex]n_{CO_2}=1.183[/tex]
The same will be the number of moles of carbon atom. Now, the number of carbon atoms can be calculated as follows
[tex]number of atoms = n_{C} \times N_A[/tex]
Here, NA is the Avogadro's number, and its value is 6.022 x 10²³. Placing the values we get:
[tex]number of atoms = 1.183 \times 6.022 \times 10^{23}\\number of atoms = 7.124 \times 10^{23}[/tex]
The number of carbon atoms in 52.06 g of CO₂ is 7.124 x 10²³ atoms
Calculation of the number of carbon atoms:
Since The molar mass of CO2 is 44.01 g/mol.
Here the mass of CO2 is
= mass / molecular mass
= 52.06 / 44.01
= 1.183
Now the number of carbon atoms should be
= 1.183 * 6.022 * 10^23
= 7.124 x 10²³
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