Question

From the equation C(s)+O2(g)----->Co2(g) find number of Co2 molecules formed when 24g of carbon is burnt in adequate oxygen?​

Answer 1

Answer:

this is your required answer

Answer 2

The total number of CO2 molecules eventually formed is 1.2023 × $10^{24}$.

Given:

Mass of carbon burnt = 24 grams.

To Find:

The number of CO2 molecules formed when 24 grams of carbon is burnt in sufficient oxygen supply =?

Solution:

We know,

The molecular mass of CO2 = 12 + 2 × 16

∴ The molar mass of CO2 = 44.

Also,  $N_{A}$ = Avogadro's Number is = 6.023 × $10^{23}$.

When Carbon (C) is burnt in the air, it reacts with the oxygen (O2) present in the air to produce Carbon Dioxide (CO2) as follows;

C (s) + O₂ (g)  -----------> CO₂ (g)

According to the chemical equation above,

When 1 mole of Solid Carbon is burnt in a sufficient supply of oxygen; we get 1 mole of Carbon Dioxide gas.

i.e., When 12 grams of Solid Carbon is burnt in the air; we get 44 grams of CO2 gas.

Now, when 24 grams of Carbon is burnt in the air; 88 grams of carbon dioxide gas will be released.

We have,

Mass of CO2 released = 88 grams.

Number of molecules of CO2 released = Number of moles of CO2 × $N_{A}$

∴ The number of molecules of CO2 released =  $\frac{Mass of CO2}{Molar Mass of CO2}$  × $N_{A}$

∴ The number of molecules of CO2 released = $\frac{88}{44}$ × 6.023 × $10^{23}$

∴ The number of molecules of CO2 released = 2  × 6.023 × $10^{23}$

∴ The number of molecules of CO2 released = 1.2023 × $10^{24}$.

Thus, The number of CO2 molecules formed when 24 grams of carbon is burnt in sufficient oxygen supply is 1.2023 × $10^{24}$.

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