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 kJA.-2820 kJB.-1410 kJC.1410 kJD.2820 kJSUBMITarrow_backPREVIOUS
Question
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 kJA.-2820 kJB.-1410 kJC.1410 kJD.2820 kJSUBMITarrow_backPREVIOUS
Solution
To solve this problem, you need to follow two steps:
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Reverse the reaction: When you reverse a reaction, the sign of the enthalpy change also reverses. So, if the enthalpy of the given reaction is -1410 kJ, when reversed, the enthalpy will be +1410 kJ.
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Multiply the reaction by 2: When you multiply the reaction by a factor, the enthalpy change also gets multiplied by the same factor. So, if the reversed reaction has an enthalpy change of +1410 kJ, when multiplied by 2, the enthalpy will be 2 * 1410 kJ = 2820 kJ.
So, the final value for the enthalpy of the reaction you use for this intermediate reaction would be 2820 kJ. Therefore, the answer is D. 2820 kJ.
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