When 1.98 g of NaOH (molar mass= 40 g/mole) are added to 75.0 mL of a 0.350 M HCl solution in a coffee-cup calorimeter, the temperature changes from 21.7°C to 25.8°C. If the resulting solution has a mass of 78.2 grams and a specific heat capacity of 3.97 J/g°C, what is the enthalpy change (ΔHrxn) for this reaction in kJ/mole.

(ΔHrxn) = 1.273kJ/mol

Explanation:

Applying

m=78.2, c= 3.97, ∆t= 25.8-21.7

(ΔHrxn)= mc∆t

=78.2× 3.97× 4.1= 1.273kJ/mol

може ли да зареждате повече информация, моля

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.