What is the enthalpy for reaction 1 reversed?
reaction 1 reversed:
2CO2+3H2O=C2H5OH+3O2
express the answer in kJ/mol
To determine the enthalpy change of the reaction 1 reversed, you will need the enthalpy change (ΔH) of the forward reaction.
If you have the value of ΔH for the forward reaction, you can use the fact that the enthalpy change of a reaction is the same whether the reaction is in the forward or reverse direction.
However, if you do not have the value of ΔH for the forward reaction, you would need to calculate it using Hess's Law or other thermodynamic data.
Hess's Law states that if you can express the desired reaction as a sum of two or more reactions, then the enthalpy change for the desired reaction is equal to the sum of the enthalpy changes of the individual reactions.
In this case, you can convert the given reaction into a sum of known reactions by reversing the direction of the given reaction and multiplying the enthalpy change by -1. The resulting reaction can be expressed as follows:
C2H5OH + 3O2 → 2CO2 + 3H2O
Now, if you know the enthalpy change (ΔH) for this reaction, you can simply multiply it by -1 to get the enthalpy change for the reaction 1 reversed.
Finally, express the enthalpy change of reaction 1 reversed in kJ/mol, which means you divide the value of ΔH by the stoichiometric coefficient of the target compound (C2H5OH in this case).
To find the enthalpy for reaction 1 reversed, you need to reverse the sign of the enthalpy change.
Given reaction 1:
2CO2 + 3H2O = C2H5OH + 3O2
If the enthalpy change for reaction 1 is denoted as ΔH, then the enthalpy change for the reverse reaction would be -ΔH. This means that the enthalpy change for the reverse reaction is equal in magnitude but opposite in sign to the original reaction.
Therefore, the enthalpy change for reaction 1 reversed is -ΔH.
Keep in mind, however, that to calculate the exact value of ΔH, you would need experimental data or thermodynamic calculations.