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Using this equation, $\ce{CaCl2(s) -> Ca^{2+}(aq) + 2Cl^{-}(aq)}$

and $\Delta H = - 325.0 \; kJ $

If you have 15.0 grams of the solid, how much heat is released or gained in kilojoules?

enter image description here

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  • $\begingroup$ Are you sure you have the right units for $\Delta H$? $\endgroup$
    – LDC3
    Commented Apr 20, 2014 at 20:54
  • $\begingroup$ @ldc3 Ya, it was a given value for the problem. $\endgroup$
    – EmptyStuff
    Commented Apr 20, 2014 at 20:58
  • $\begingroup$ Suppose you dissolve a gram of calcium chloride and then a kilogram, both in excess water. They cannot each and both be the value you posted. If you have the correct units, the path to a correct answer is obvious. Open your textbook. The first time you do it there is a crackling sound. Google it, "enthalpy of solution". BTW, the value is for infinite dilution. $\endgroup$
    – Uncle Al
    Commented Apr 20, 2014 at 21:03
  • $\begingroup$ $\Delta H$ is usually in $kJ/mol$. That is why I am asking. Either the question has a mistake or maybe it is $\Delta H^°$ $\endgroup$
    – LDC3
    Commented Apr 20, 2014 at 21:03
  • $\begingroup$ @LDC3 I updated the post with a picture of the question. It very may well be kJ/mol but it isn't stated. $\endgroup$
    – EmptyStuff
    Commented Apr 20, 2014 at 23:06

1 Answer 1

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I'm going to assume that the question is presenting the given change in enthalpy as a molar enthalpy change (so as to say that -325.0 kJ are evolved per mole of CaCl2).

Under that assumption, answering the question is then a matter of using the a molar fraction of CaCl2 for the amount you have present.

CaCl2 has a molar mass of 110.98 g/mol so with 15.0 g of CaCl2, you'd have roughly 0.1352 mol of CaCl2. 0.1352 mol * -325.0 kJ/mol = -43.94 kJ. The negative here means that the CaCl2 will release 43.94 kJ of heat.

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