Thursday

April 24, 2014

April 24, 2014

Posted by **a Canadian** on Thursday, February 21, 2013 at 5:16pm.

One of the options was that there was insufficient information because you need the mass of H2O used to cool the aluminum.

I chose that one... Is that right?

I chose it because I remember my teacher explaining that when you have a solid and a solution reacting, you only use the mass of the solution when doing Q=mc(detlaT). She said, "to explain it simply... What are you putting the thermometer in? The solid or the solution? You're not going to stick a thermometer into a solid." So I thought you'd need the mass of H2O because you can't use the mass of Al... But I overheard other people talking about it and I think a bunch of people calculated an actual value...

I just want to know if I got it right or wrong; it's been bugging me all day.

- Chemistry -
**DrBob222**, Thursday, February 21, 2013 at 5:31pm"Something like" isn't enough for me to know.

q = mass Al x specific heat Al x (Tfinal-Tinitial)

If you used H2O to cool the Al you would need the mas of the H2O and the initial T of the H2O, then you could do the final T. Of course the final T of the water will be the same as the final T of the Al.

- Chemistry -
**bobpursley**, Thursday, February 21, 2013 at 5:31pmenthlapy = heat change.

enthalpy change=mass*specheat*deltaTemp

- Chemistry -
**a Canadian**, Thursday, February 21, 2013 at 5:41pmThanks; I obviously got it wrong, but what was my teacher talking about when she said that when you have a solid reacting, you don't use the mass of the solid for Q=mc(deltaT), only the mass of liquids or solutions? Why wouldn't that apply in this case?

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