Respuesta :
Answer: The correct answer is 1.18 g.
Explanation:
We are given a chemical equation:
[tex]C(S)+O2(g)\rightarrow CO_2(g)[/tex]
We know that at STP conditions:
22.4L of volume is occupied by 1 mole of a gas.
So, 2.21L of carbon dioxide is occupied by = [tex]\frac{1}{22.4L}\times 2.21L=0.0986mol[/tex] of carbon dioxide gas.
By Stoichiometry of the above reaction:
1 mole of carbon dioxide gas is produced by 1 mole of carbon
So, 0.0986 moles of carbon dioxide is produced by = [tex]\frac{1}{1}\times 0.0986=0.0986mol[/tex] of carbon.
Now, to calculate the mass of carbon, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Moles of carbon = 0.0986 mol
Molar mass of carbon = 12 g/mol
Putting values in above equation, we get:
[tex]0.0986mol=\frac{\text{Mass of carbon}}{12g/mol}\\\\\text{Mass of carbon}=1.18g[/tex]
Hence, the correct answer is 1.18 g.
Answer: The mass of carbon burned in oxygen at STP is 1.18 grams.
Explanation:
At STP:
22.4 L of volume is occupied by 1 mole of gas
We are given:
Volume of carbon dioxide = 2.21 L
So, moles of carbon dioxide gas will be = [tex]\frac{2.21}{22.4}=0.0987mol[/tex]
For the given chemical reaction:
[tex]C(s)+O_2(g)\rightarrow CO_2(g)[/tex]
By Stoichiometry of the reaction:
1 mole of carbon dioxide gas is formed when 1 mole of carbon is reacted.
So, 0.0987 moles of carbon dioxide is formed when [tex]\frac{1}{1}\times 0.0987=0.0987mol[/tex] of carbon id reacted.
Now, calculating the mass of carbon by using equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Molar mass of carbon = 12 g/mol
Moles of carbon = 0.0987 moles
Putting values in above equation, we get:
[tex]0.0987mol=\frac{\text{Mass of carbon}}{12g/mol}\\\\\text{Mass of carbon}=(0.0987mol\times 12g/mol)=1.18g[/tex]
Hence, the mass of carbon burned in oxygen at STP is 1.18 grams.
