Two water solutions that have a density of 1.00 g/mL are mixed, and a reaction occurs.
The temperature rises from 25.0°C to 27.0°C.
Given that the heat capacity is 4.18 J/g x°C
and that the total mass of the water is 75.0 g,
what is the heat change for the reaction?

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.

the answer is the first option

explanation:

just googled it m8. not that hard

lol