How To Find Molar Heat Of Solution

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Molar Heat of Solution

• Thread starter Christina-
• Start date Mar 17, 2007

Homework Argument

When v.00 thou of NaOH_(s) are added to 100 k of water using a calorimeter (with Cp = 493.24 J/One thousand), the temperature rises from 25.0 to 37.five °C. Summate the tooth heat of solution.
[marshal=center]NaOH(s)--->Na_(aq)+OH_(aq)[/align]
Assume that the specific oestrus capacity of h2o is four.eighteen J/gK and that of the NaOH_(aq) solution is the same.

Homework Equations

1) q_p = C_p∆T,
2) | Rut Lost by Hot H2o | = | Heat Gained by Cold Water | + | Heat Gained By Calorimeter |

The Attempt at a Solution

Estrus Gained By Solution:
(100 g H_iiO) x (iv.18 J/gK) x (37.5 - 25)K = 5486.25 JOestrus Gained By Calorimeter:
Using q_p = C_p∆T,
C_p∆T = (493.24 J/1000) x (37.v - 25)K = 6165.5 J

| Heat Lost | = 5486.25 J + 6165.5 J = 11 651.75 J = 11.65175 kJ

Molar mass of NaOH = (22.99 + 16.00 + 1.01) = 40
v.00 g NaOH x (i mol ÷ 40g) = 0.125 mol

11.65175 kJ ÷ 0.125 mol =

93.214 kJ/mol

I was only wondering if I did that correctly. I don't actually know the correct answer, only 1 of my young man students got a different reply and I'm unsure if I'g the ane with the wrong answer or not.
If this isn't the way to find ∆H, could someone show me how or perchance point me to a useful page on the internet?

Thanks

Answers and Replies

One pocket-sized thing I tin can see immediately

you wrote;
(100 one thousand Water) x (4.eighteen J/gK) x (37.5 - 25)Thousand = 5486.25 J
only this should actually be;
(100 one thousand H2O) x (4.18 J/gK) x (37.5 - 25)Grand =

5225 J
or
(105 thousand Water) x (four.eighteen J/gK) x (37.5 - 25)K = 5486.25 J

I don't know if this helps but information technology's what I could meet immediately

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