Question

The DH for the solution process when solid sodium hydroxide dissolves in water is -44.4 kJ/mol. When a 13.9-g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0 C to ________ C. Assume that the solution has the same specific heat as liquid water, i.e., 4.18 J/g-K

Answer 1

Answer:

The temperature increases from 23.0 C to 37.0 °C

Explanation:

Step 1: Data given

DH = -44.4 kJ/mol

mass NaOH = 13.9 grams

mass of water = 250.0 grams

Initial temperature = 23°C = 295 K

Final temperature = TO BE DETERMINED

Specific heat = 4.18 J/g*K

Step 2: Calculate change in temperature

13.9 grams/ 40 g/mol * 44.4 kJ/mol = 15429 J

15429 J = (massNaOH + mass water) * 4.18 * ΔT

15429 = 263.9 *4.18 * ΔT

ΔT = 14°C

Step 3: Calculate final temperature

ΔT= 14°C = T2 - 23°C

T2 = 23 +14 = 37 °C

The temperature increases from 23.0 C to 37.0 °C

Answer 2

Answer:

The temperature increases from 23.0°C to 37.76°C

Explanation:

please look at the solution in the attached Word file

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