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If you need to reverse the following reaction and multiply it by 2 in order for it to be an intermediate reaction in a Hess's law problem, what would be the final value for the enthalpy of reaction you use for this intermediate reaction? C2H4 + 3 O2 2 CO2 + 2 H2O, H = -1410 kJ

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The reaction is:
C₂H₄ + 3O₂ → 2CO₂ + 2H₂O; ΔH = 1410 kJ

When we reverse this reaction, the sign of the enthalpy  change, ΔH, will be changed. The enthalpy change for the reversed reaction would be 1,410 kJ.
Next, we must also multiply the reaction by 2, so the final enthalpy change for the reverse reaction will be:

ΔH = 2,820 kJ
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When turned around, the equation is  4 CO2 + 4 H2O -----> 4C2H4 + 6 O2  ΔH = 2820 kJ.

What is Hess law?

The Hess law of constant heat summation can be used to obtain the total of all the heat changes that took place in a process by summation.

For the reaction; C2H4 + 3 O2 ----> 2 CO2 + 2 H2O, ΔH= -1410 kJ, when turned around and multiply by 2, we have; 4 CO2 + 4 H2O -----> 4C2H4 + 6 O2  ΔH = 2820 kJ. We must note that the change in the sign of ΔH is because the reaction equation has been turned around.

Learn more about Hess law: https://brainly.com/question/867780