I need some help with a Chemistry/Physics problem, just need to be put in right direction (no answer)?

Question

We are in the thermochemistry portion of class and I missed a lecture so Im a bit behind and don't know if Im solving this correctly.

Here is the question given: When 4.21 g of hydroxide are added to 250ml of water, the temperature rises 4.14(C). Assume that the density and specific heat of the dilute aqueous solutions are the same as those of H2O and calculate the molar heat of solution of potassium hyroxide.

Ok I think Im getting confused with the term "molar heat".

Do I basically use the q=MC(delta)T?

Add grams of water and grams of KOH together and solve for q?

Then divide the J I get into moles of KOH?

Or would I use q of solution=-q of reactants?

Please dont do it for me I just need a step in the right direction. Any help would be appreciated.

Answer 1

Divide the joules of heat that you get (using q = mc delta T) by the moles of KOH - not into the moles of KOH!

It is most important that you realise that the reaction is exothermic, so that a negative sign should be inserted into your final answer.

Answer 2

Assuming the 4.21g of OH means 4.21 g of KOH?
You look up the specific heat capacities of KOH and H2O
Take care with the units.
Delta T *Σ(CiMi) = J ▐ if Ci =Cw, Ck are the specific heats of water and KOH respecively and IF the C's are in units of joules per mole per degree kelvin then the Ms are the moles of the two OR if the C's are in units of joules per gram per degree kelvin then the M's are the mass (in grams).
The molar heat is the number of joules per mole of KOH so it is just a proportion to the 4.21 (?) grams of KOH (?) you have data for. Once you figure the energy released its easy to figure knowing the number of moles 4.21 grams is.

Answer 3

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