What happens when ethanol is heated with excess concentrated sulfuric acid at 443 K? Write the chemical equation for the reaction, state the role of concentrated sulfuric acid in this reaction, and calculate the volume of carbon dioxide gas produced at Standard Temperature and Pressure (STP) when 4.6 grams of ethanol undergoes complete combustion.

Q: What happens when ethanol is heated with excess concentrated sulfuric acid at 443 K? Write the chemical equation for the reaction, state the role of concentrated sulfuric acid in this reaction, and calculate the volume of carbon dioxide gas produced at Standard Temperature and Pressure (STP) when 4.6 grams of ethanol undergoes complete combustion.

Part 1: Dehydration of Ethanol\nWhen ethanol is heated with excess concentrated sulfuric acid ($H2SO4$) at 443 K, it undergoes dehydration (loss of a water molecule) to form ethene gas. Chemical Equation: $$CH3CH2OH \xrightarrow443\text{ K}{\text{Conc. } H2SO4} CH2=CH2 + H2O$$ Role of Concentrated Sulfuric Acid:\nConcentrated sulfuric acid acts as a dehydrating agent in this reaction, meaning it has a strong affinity for water and removes a molecule of water from the ethanol molecule. --- Part 2: Combustion Numerical Problem Given Data: Mass of ethanol ($C2H5OH$) burned = $4.6\text{ g}$ Molar mass of Carbon ($C$) = $12\text{ g/mol}$ Molar mass of Hydrogen ($H$) = $1\text{ g/mol}$ Molar mass of Oxygen ($O$) = $16\text{ g/mol}$ Step 1: Calculate the molar mass of ethanol ($C2H5OH$) $$\text{Molar mass} = (2 \times 12) + (6 \times 1) + (1 \times 16) = 24 + 6 + 16 = 46\text{ g/mol}$| Step 2: Calculate the number of moles of ethanol $$\text{Moles of } C2H5OH = \frac{\text{Given mass}}{\text{Molar mass}} = \frac{4.6\text{ g}}{46\text{ g/mol}} = 0.1\text{ moles}$$ Step 3: Write the balanced chemical equation for the combustion of ethanol $$C2H5OH + 3O2 \rightarrow 2CO2 + 3H2O$$ Step 4: Determine the molar ratio between ethanol and carbon dioxide\nFrom the balanced equation: $1\text{ mole}$ of $C2H5OH$ produces $2\text{ moles}$ of $CO2$. Therefore, $0.1\text{ moles}$ of $C2H5OH$ will produce: $$\text{Moles of } CO2 = 0.1 \times 2 = 0.2\text{ moles}$$ Step 5: Calculate the volume of $CO2$ at STP\nAt Standard Temperature and Pressure (STP), $1\text{ mole}$ of any ideal gas occupies $22.4\text{ liters}$. $$\text{Volume of } CO2 = \text{Moles of } CO2 \times 22.4\text{ L/mol}$$ $$\text{Volume of } CO2 = 0.2\text{ mol} \times 22.4\text{ L/mol} = 4.48\text{ liters}$$

Question

Accepted Answer

Part 1: Dehydration of Ethanol
When ethanol is heated with excess concentrated sulfuric acid ($H2SO4$) at 443 K, it undergoes dehydration (loss of a water molecule) to form ethene gas. Chemical Equation: $$CH3CH2OH \xrightarrow443	ext{ K}{	ext{Conc. } H2SO4} CH2=CH2 + H2O$$ Role of Concentrated Sulfuric Acid:
Concentrated sulfuric acid acts as a dehydrating agent in this reaction, meaning it has a strong affinity for water and removes a molecule of water from the ethanol molecule. --- Part 2: Combustion Numerical Problem Given Data: Mass of ethanol ($C2H5OH$) burned = $4.6	ext{ g}$ Molar mass of Carbon ($C$) = $12	ext{ g/mol}$ Molar mass of Hydrogen ($H$) = $1	ext{ g/mol}$ Molar mass of Oxygen ($O$) = $16	ext{ g/mol}$ Step 1: Calculate the molar mass of ethanol ($C2H5OH$) $$	ext{Molar mass} = (2 	imes 12) + (6 	imes 1) + (1 	imes 16) = 24 + 6 + 16 = 46	ext{ g/mol}$| Step 2: Calculate the number of moles of ethanol $$	ext{Moles of } C2H5OH = \frac{	ext{Given mass}}{	ext{Molar mass}} = \frac{4.6	ext{ g}}{46	ext{ g/mol}} = 0.1	ext{ moles}$$ Step 3: Write the balanced chemical equation for the combustion of ethanol $$C2H5OH + 3O2 ightarrow 2CO2 + 3H2O$$ Step 4: Determine the molar ratio between ethanol and carbon dioxide
From the balanced equation: $1	ext{ mole}$ of $C2H5OH$ produces $2	ext{ moles}$ of $CO2$. Therefore, $0.1	ext{ moles}$ of $C2H5OH$ will produce: $$	ext{Moles of } CO2 = 0.1 	imes 2 = 0.2	ext{ moles}$$ Step 5: Calculate the volume of $CO2$ at STP
At Standard Temperature and Pressure (STP), $1	ext{ mole}$ of any ideal gas occupies $22.4	ext{ liters}$. $$	ext{Volume of } CO2 = 	ext{Moles of } CO2 	imes 22.4	ext{ L/mol}$$ $$	ext{Volume of } CO2 = 0.2	ext{ mol} 	imes 22.4	ext{ L/mol} = 4.48	ext{ liters}$$

Part 1: Dehydration of Ethanol\nWhen ethanol is heated with excess concentrated sulfuric acid ($H_2SO_4$) at 443 K, it undergoes dehydration (loss of a water molecule) to form ethene gas.

Part 2: Combustion Numerical Problem