441.7 kJ/mol is the delta H (in kJ/mol NaOH) for the solution process. When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 21.6 °C to 37.8 °C.
The specific heat capacity is defined as the quantity of heat (J) absorbed per unit mass (kg) of the material when its temperature increases 1 K (or 1 °C), and its units are J/(kg K) or J/(kg °C).
Specific heat of water = 4.18 J/g °C
Total mass = 100 + 6.5 = 106.5 g
Q = mCpΔT
Q = 106.5 x 4.18 x (37.8 - 21.6)
Q = 7177 Joules
Moles of NaOH:
Moles = [tex]\frac{mass}{molar \;mass}[/tex]
Moles = [tex]\frac{6.5}{23 + 16 + 1}[/tex]
= 0.1625
Enthalpy of reaction: [tex]\frac{7177}{0.1625}[/tex]
= 441.7 kJ/mol NaOH
Hence, 441.7 kJ/mol is the delta H (in kJ/mol NaOH) for the solution process. When a 6.50-g sample of solid sodium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 21.6 °C to 37.8 °C.
Learn more about specific heat capacity here:
https://brainly.com/question/1747943
#SPJ5
