contestada

A 0.534 g sample of steam at 104.3 ∘C is condensed into a container with 4.86 g of water at 15.9 ∘C. What is the final temperature of the water mixture if no heat is lost? The specific heat of water is 4.18 J g⋅ ∘C, the specific heat of steam is 2.01 J g⋅ ∘C, and Δvap=40.7 kJ/mol.

Respuesta :

pstnonsonjoku

The final temperature of the water is 75.6∘C.

What is condensation?

Condensation is the process by which steam is  converted to water at the boiling point of water. Heat lost by steam = Heat gained by water.

Heat lost by steam= ( 0.534 g × 2.03 × (104 - 100)) + (0.534 g × 40.7 × 10^3 / 18) = 4.34 + 1207.4 = 1211.74 J

Heat gained by water = ( 4.86  × 4.18 × (T2 - 15.9 ∘C))

1211.74  = 20.3T2 - 322.77

1211.74 + 322.77 = 20.3T2

T2 = 1211.74 + 322.77/20.3

T2 = 75.6∘C

Learn more about specific heat capacity: https://brainly.com/question/2530523

Otras preguntas