Respuesta :
Answer:
So there is83.6g CO2 produced
Explanation:
Burning carbon with air has the following equation
C + O2 → CO2
For 1 mol Carbon, we have 1 mol O2 and 1 mol CO2
Step 2: Calculating moles
mole C = 22.8g / 12g/mole
Mole C = 1.9 mole
1.9 mole C will completely react
Since for each mole C there is 1 mole O2 and 1 mole CO2
This means there will also react 1.9 mole of 02, to be formed 1.9 mole of CO2
mole CO2 = mass CO2 / Molar mass CO2
mass CO2 = 1.9 mole CO2 * 44g/mole =83.6g CO2
In this reaction 18.2 g of O2 remained unreacted
we can control this: 79g - 18.2 g = 60.8g
1.9 mole * 32g/mol = 60.8g
So there is83.6g CO2 produced
83.6g of [tex]\rm CO_{2}[/tex] will be produced.
When the carbon dioxide reacts with the oxygen to yield carbon dioxide then the reaction is called the combustion reaction and heat or light is also produced in the form of flames.
How to calculate the mass of carbon dioxide?
Given,
- Mass of Carbon = 22.8 g
- The total mass of the Oxygen atom = 79.0 g
- Mass of the unreacted oxygen = 18.2 g
- Mass of the [tex]\rm CO_{2}[/tex] = ?
The reaction can be shown as,
[tex]\rm C + O_{2} \rightarrow \rm CO_{2}[/tex]
Calculate the moles of carbon:
[tex]\begin{aligned}\rm Moles (n) &= \dfrac{\rm mass}{\rm molar \;mass}\\\\\rm n &= \dfrac{22.8}{12}\\\\\rm n &= 1.9 \;\rm mol\end{aligned}[/tex]
1 mole of oxygen = 1 mole of carbon dioxide
So, 1.9 moles of oxygen will be needed for 1.9 moles of carbon dioxide
Mass of carbon dioxide will be calculated as:
[tex]\begin{aligned}\rm Mass (m) &= \rm moles \times \rm molar \; mass\\\\&= 1.9 \times 44\\\\&= 83.6 \;\rm g\end{aligned}[/tex]
Since, 18.2 g of oxygen is left unreacted, therefore:
[tex]\begin{aligned}&=79 \;\rm g - 18.2 \;\rm g\\\\&= 60.8\;\rm g\end{aligned}[/tex]
Can also be calculated as,
[tex]\begin{aligned}\rm Mass &= 1.9 \;\rm moles \times 32 \;\rm g/mol\\\\&= 60.8\;\rm g \end{aligned}[/tex]
Therefore, 83.6g of [tex]\rm CO_{2}[/tex] will be produced.
Learn more about combustion reaction here:
https://brainly.com/question/13385740
