# Problem: A 100.0-mL sample of 0.662 M KOH is mixed with a 100.0-mL sample of 0.662 M HNO3 in a coffee cup calorimeter. If both solutions were initially at 30.64°C and the temperature of the resulting solution was recorded as 35.15°C, determine the ΔH°rxn for the neutralization reaction between aqueous KOH and HNO3. Assume that no heat is lost to the calorimeter or the surroundings, and that the density and the heat capacity of the resulting solution are 1.00 g/mL and 4.18 J/(g°C), respectively.A) -27.9 kJ B) -57.0 kJ C) -16.7 kJ D) - 34.4 kJ E) -169 kJ

###### FREE Expert Solution

Use the concept of calorimetry to determine the heat of neutralization between KOH and HNO3

For this problem, follow the steps:

1. Determine the total mass of solution

2. Calculate change in temperature

3. Determine the amount of heat released

4. Calculate the heat of enthalpy

The neutralization reaction of KOH(aq) and HNO3(aq) is

KOH(aq) + HNO3(aq) → KNO3(aq) + H2O(l) ###### Problem Details

A 100.0-mL sample of 0.662 M KOH is mixed with a 100.0-mL sample of 0.662 M HNO3 in a coffee cup calorimeter. If both solutions were initially at 30.64°C and the temperature of the resulting solution was recorded as 35.15°C, determine the ΔH°rxn for the neutralization reaction between aqueous KOH and HNO3. Assume that no heat is lost to the calorimeter or the surroundings, and that the density and the heat capacity of the resulting solution are 1.00 g/mL and 4.18 J/(g°C), respectively.

A) -27.9 kJ

B) -57.0 kJ

C) -16.7 kJ

D) - 34.4 kJ

E) -169 kJ