calculate the delta h for the reaction 2C+2H--> C2H4
C+O2--> Co2 delta h= -393.5
C2H4+ 3O2--> 2CO2+ 2H2O delta h= 1410.9
H2+ 1/2 O2--> H2O delta h= -285.8
2CO+ O2--> 2CO2 delta h= -566.0
do you flip the first two equations and times the first and third one by 2?
To calculate the ΔH for a reaction, you need to consider the stoichiometric coefficients of the reactants and products involved. In this case, let's calculate the ΔH for the reaction:
2C + 2H2 -> C2H4
The given information provides the ΔH values for several other reactions. However, to calculate the ΔH for the given reaction, you cannot simply flip or multiply the existing reactions.
To determine the ΔH for the desired reaction, you can use Hess's Law, which states that the ΔH for a reaction is equal to the sum of the ΔH values for the individual reactions that lead to that reaction, as long as the reactions are multiplied by appropriate coefficients.
Here's how you can use Hess's Law to calculate the ΔH for the given reaction:
1. Multiply the first equation by 2:
2C + 2O2 -> 2CO2 (ΔH = 2 x (-393.5) = -787.0)
2. Multiply the third equation by 2:
H2 + O2 -> 2H2O (ΔH = 2 x (-285.8) = -571.6)
3. Combine the equations:
-787.0 + -571.6 = -1358.6
4. Flip the sign of the ΔH value, as the reaction is reversed:
ΔH = +1358.6
Therefore, the ΔH for the reaction 2C + 2H2 -> C2H4 is +1358.6 kJ/mol.