is this the answer to B )
CH3CH2OH + 3O2 → 2CO2 + 3H2O
In winemaking, the sugars in grapes undergo fermentation by yeast to yield CH3CH2OH and CO2. During cellular respiration, sugar and ethanol are "burned" to water vapor andCO2.
Write a combustion reaction for ethanol. INCLUDE PHYSICAL STATES
I need help with balancing the equation
i think it's
CH3CH2OH + 3O2 → 2CO2 + 3H2O
then it said HINT:
Start by writing a balanced chemical equation for the fermentation reaction of C6H12O6 and for the respiration reaction (combustion) of C6H12O6...what formula should be used to find the standard enthalpy of a reaction? Use the standard enthalpy of formation values from your textbook when calculating the standard enthalpy of reaction for both fermentation and respiration. thanks!• INCLUDE PHYSICAL STATES
The balanced chemical equation for the fermentation reaction of C6H12O6 is C6H12O6 → 2CH3CH2OH + 2CO2.
The balanced chemical equation for the respiration reaction (combustion) of C6H12O6 is C6H12O6 + 6O2 → 6CO2 + 6H2O.
The formula used to find the standard enthalpy of a reaction is ΔH = ΣΔHf (products) - ΣΔHf (reactants).
To write a balanced combustion reaction for ethanol (CH3CH2OH), you need to ensure that the number of atoms on each side of the equation is equal. Here's the balanced equation:
C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(g)
In this equation:
- "l" represents the liquid state of ethanol.
- "g" represents the gaseous state of oxygen, carbon dioxide, and water.
Regarding the hint, the formula you should use to find the standard enthalpy of a reaction is:
ΔH° = ΣnΔH°f(products) - ΣnΔH°f(reactants)
In this formula,
- ΔH° represents the standard enthalpy of reaction
- ΣnΔH°f(products) represents the sum of the standard enthalpy of formation of all products, where n is the stoichiometric coefficient
- ΣnΔH°f(reactants) represents the sum of the standard enthalpy of formation of all reactants, where n is the stoichiometric coefficient
This formula allows you to calculate the standard enthalpy of a reaction using the standard enthalpy of formation values from your textbook.
To write a balanced combustion reaction for ethanol (CH3CH2OH), we need to ensure that both sides of the equation have the same number of atoms for each element. Here's how we can balance the equation:
1. Start with the unbalanced equation: CH3CH2OH + O2 → CO2 + H2O
2. Count the number of atoms for each element on both sides of the equation:
- Carbon (C): 2 on the left, 1 on the right
- Hydrogen (H): 6 on the left, 2 on the right
- Oxygen (O): 1 on the left (from the CH3CH2OH molecule), 2 on the right (from the CO2 molecule) + x on the right (from the H2O molecule), where x is the number of oxygen atoms needed to balance oxygen.
3. Balance the carbon and hydrogen atoms first:
- Add a coefficient of 2 in front of CO2: CH3CH2OH + O2 → 2CO2 + H2O
- Add a coefficient of 3 in front of H2O: CH3CH2OH + O2 → 2CO2 + 3H2O
4. Balance the oxygen atoms:
- Since there are 9 oxygen atoms on the right side (2 from CO2 + 3x from H2O) and only 1 on the left side, we need 8 additional oxygen atoms on the left side to balance the equation.
- Add a coefficient of 4 in front of O2: CH3CH2OH + 4O2 → 2CO2 + 3H2O
The balanced equation for the combustion of ethanol with physical states included is:
C2H5OH(ℓ) + 4O2(g) → 2CO2(g) + 3H2O(ℓ)
The hint about using the standard enthalpy of formation values suggests that you can calculate the standard enthalpy of the reaction using the standard enthalpy of formation values from your textbook. The standard enthalpy of formation (ΔHf°) is the change in enthalpy when one mole of a compound is formed from its constituent elements in their standard states. By subtracting the sum of the standard enthalpies of formation of the reactants from the sum of the standard enthalpies of formation of the products, you can calculate the ΔH° for the reaction.