Question

For the theoretical (theory/moles used), how do we get the "moles used"

CALORIMETRY, Heat evolution from HCI+NaOH H+ ?? , H2O +AH (-70.3 kJ/mole) given value black-input, red CALC,blue-given + Volume HCI Density HCI mass HCI Molarity HCI 50.0 1.018 50.90 1.00 0.050 mL g/mL gramrs mole/L moles (mL 1000) L Volume NaOH 50.0 L Density NaOH 1.044 mass NaOH 52.20 1.50 (mL / 1000) m/L 0.075 moles of limiting reactant0.050 g/ml grams mole /L moles mole gramms Molarity NaOH Mass of mixture 103.100 o°C J/(°C-gram) Joule s Joulelmol Joule s Joules Jouler C 6.65 AT at T-0, maximum from graph Specific heat of mix (given value) (4.058) -mrAT Cp (Cp specific heat)(2,782) The oretical energy release (given) (70,300) Theoretical theoryI moles used (3,515) difference theory-actual 33) diff I degree-calorimeter const. 1 110.2

Answer 1

Ans. Moles used = Molarity x Volume of solution in liters

For example, amount of HCl taken = 50.0 mL of 1.00 M molarity.

Now,

            Moles of HCl used = 1.00 M x 0.050 L = 0.050 mol

# Theoretical value of “q” =

Theoretical enthalpy of neutralization x Moles of limiting reactant (HCl)

= (70300 J / mol) x 0.050 mol

= 3515.0 J