How much energy is released or absorbed when 40.0 g of steam at 250.0 c is converted to water at 30.0 c?

The steam needs to condense, which occurs at 100C- 1. Q = (40.0g)(2.031J/gC)(250C-100C) The phase change is occurs- 2. Q = (40.0g)(79.72 cal/g) The water cools from 100C to 30C 3. Q = (40.0g)(4.18J/gC)(100C-30C)

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BarrettArcher BarrettArcher · Answer 2 · 2019-05-17T09:18:00+02:00

Answer : The amount of energy released are, -36836.8 J

Solution :

Formula used :

[tex]Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})[/tex]

where,

Q = heat or energy released or absorbed = ?

m = mass of water = 40 g

c = specific heat of water = [tex]4.186J/g^oC[/tex]

[tex]\Delta T=\text{Change in temperature}[/tex]

[tex]T_{final}[/tex] = final temperature = [tex]30^oC[/tex]

[tex]T_{initial}[/tex] = initial temperature = [tex]250^oC[/tex]

Now put all the given values in the above formula, we get

[tex]Q=40g\times 4.186J/g^oC\times (30-250)^oC[/tex]

[tex]Q=-36836.8J[/tex]

The negative energy means energy is released and positive energy means energy is absorbed.

Therefore, the amount of energy released are, -36836.8 J