You have

180ml

of a drink of water at

20\\\\deg C

to which you add one ice cube of

30.5ml

volume at

-18\\\\deg C

. Assuming no heat exchange with the environment, at what temperature will your drink be after equilibrium is reached?\

C_(sol )=2.09Jg^(-1)K^(-1),C_(liq )=4.18Jg^(-1)K^(-1)\ \\\ ho _(sol )=0.917gcm^(-3),\\\ ho _(liq )=0.9937gcm^(-3)\ \\\\Delta _(fus )H^(0)=6.02kJmol^(-1),M=18.02gmol^(-1)

\ A.

7.499\\\\deg C

\ B.

7.50\\\\deg C

\ C.

6.09\\\\deg C

\ D.

6.49\\\\deg C

\ E.

5.27\\\\deg C

\ Source: Flickr/Kristian Urdal: CC BY-NC-SA

You have 180ml of a drink of water at 20C to which you add one ice cube of 30.5ml volume at 18C. Assuming no heat exchange with the environment, at what temperature will your drink be after equilibrium is reached? Csol=2.09Jg1K1sol=0.917gcm3fusH0=6.02kJmol1Cliq=4.18Jg1K1liq=0.9937gcm3M=18.02gmol1 A. 7.499C B. 7.50C C. 6.09C D. 6.49C E. 5.27C Source: Flickr/Kristian Urdal: CC BY-NC-SA