What is the molarity of a Stock solusion of sugar (Sucrose, C12H22O11) syrup made with mixing 2.5 moles of sugar in 3.5 liters of water? a. 1.4 moles/ L
b. 0.71 moles
c. 0.71 M
d. None of the above

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.

1.43 x 10^-11 j the guy commented the awnser just making sure u see it .

elements make up everything, and they combine to make compounds.

the answer is c