Magnesium oxide reacts slowly with water to form magnesium hydroxide. What would be the effect on the observed value for ∆H_rxn for the reaction of MgO if 10% of the MgO had reacted with water to form Mg(OH)2? Would the value be higher or lower? (Hint: you need to determine the ∆H value for the reaction of Mg(OH)2 with HCl from heat of formation data.)
(∆H_rxn for MgO Trial 1=-72.650kJ Trial 2=-121.207kJ)
(∆H_rxn for MgO Trial 1=-72.650kJ Trial 2=-121.207kJ)
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Wouldn't it just be 10% of the average heats of the reaction?
So -9.64 kJ.
It would be a higher change in enthalpy technically, but it is less heat released; depends on how they want you to answer it.
So -9.64 kJ.
It would be a higher change in enthalpy technically, but it is less heat released; depends on how they want you to answer it.