Question

How much heat (in kJ) is required to convert 424 g of liquid H2O at 22.6°C into steam at 149°C? (Assume that the specific heat of liquid water is 4.184 J/g·°C, the specific heat of steam is 2.078 J/g·°C, and that both values are constant over the given temperature ranges. The normal boiling point of H2O is 100.0°C.)

Answer 1

The answer to your question is 1137.45 kJ

Step-by-step explanation:

Data

mass = 424 g

T1 = 22.6°C

T2 = 149°C

Clw = 4.184 J/g°C

Cv = 2.078 j/g°C

Latent heat = 2257 J/g

Process

1.- Heat of liquid

Heat = (424)(4.184)(100 - 22.6)

Heat = 137308.8 J

2.- Calculate latent heat

Latent heat = (424)(2257)

Latent heat = 956968 J

3.- Heat of vapor

Heat = (424)(2.078)(149 - 100)

Heat = 43172.5 J

4.- Total heat

Heat = 137308.8 + 956968 + 43172.5

Heat = 1137449.3 J = 1137.45 kJ