When 50.0 ml of water containing 0.50 mol hcl at 22.5°c are mixed with 50.0 ml of water containing 0.50 mol naoh at 22.5°c in a calorimeter, the temperature of the solution increases to 26.0°c. how much heat (in kj) was released by this reaction? note: the specific heat of water (cwater) is 4.18 j/(g•˚c) and the density of the solution is 1.00 g/ml.

Explanation:

Hello,

At the specified conditions, to compute the released heat due to the mixing process, which also includes the effect of the reaction enthalpy, we take into account the following formula:

All of the terms listed above are considered as changes. Thus, the enthalpy due to the water heating turns out into:

Now, it is found that the enthalpy of the carried out reaction:

Has a value of -56.72kJ/mol but as 0.5 mol are involved, the total enthalpy turns out into -28.5kJ

Now, that reaction enthalpy is by far higher than the enthalpy due to the temperature increasing, thus, one concludes that the total released enthalpy is negative and has a value of:

Best regards.

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