When a 3.23 g sample of solid sodium hydroxide was dissolved in a calorimeter in 100.0 g of water, the temperature rose from 23.9 °c to 32.0 °c. calculate δh (in kj/mol naoh) for the following solution process: naoh(s) →na+(aq)+ oh−(aq)

-41,9kJ/mol NaOH

Explanation:

For the solution process:

NaOH(s) →Na⁺(aq) + OH⁻(aq)

The released heat is:

Q = -C×m×ΔT

Where Q is the released heat, C is specific heat of the solution (4,18J/g°C), m is the mass of water (100,0g) and ΔT is (32,0°C-23,9°C)

Replacing:

Q = -3385,8J

This heat is released per 3,23g of NaOH. Now, the heat released (ΔH) per mole of NaOH is:

= -41929J/molNaOH ≡

-41,9kJ/mol NaOH

I hope it helps!

sodium (na), for example, has one electron in its valence shell. this is an unstable state because that valence shell needs eight electrons to be full. in order to fill its valence shell, find a way to add seven electrons to its valence shell

sry but any answer choices