If you need to reverse the following reaction 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?H2 + 0.5 O2 H2O, H = -286 kJA.-286 kJB.286 kJC.572 kJD.-572 kJSUBMITarrow_backPREVIOUS
Question
If you need to reverse the following reaction 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?H2 + 0.5 O2 H2O, H = -286 kJA.-286 kJB.286 kJC.572 kJD.-572 kJSUBMITarrow_backPREVIOUS
Solution
The enthalpy change of a reaction is the amount of heat absorbed or released by the reaction. In this case, the enthalpy change is -286 kJ, which means the reaction releases heat.
If you reverse the reaction, the sign of the enthalpy change also reverses. This is because reversing the reaction changes it from exothermic (releases heat) to endothermic (absorbs heat), or vice versa.
So, if you reverse the reaction H2 + 0.5 O2 -> H2O, the enthalpy change becomes -(-286 kJ) = 286 kJ.
Therefore, the final value for the enthalpy of reaction you use for this intermediate reaction would be 286 kJ.
So, the answer is B. 286 kJ.
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