[s3a]

50.0 mL of 1.00 M HCl solution are mixed with 30.0 mL of 2.00 M NaOH solution in a coffee-cup
                                                                           o
calorimeter. The initial temperature of the solutions before mixing is 20.5 C. The highest
                                           o
temperature recorded after mixing is 29.8 C. The total mass of the solution is 80.5 g. Calculate
a) the heat change, q, in joules, accompanying this reaction and state whether the process is exo- or
                                                       o                               o
endothermic b) the enthalpy of neutralization, ∆H , in kJ/mol. ( swater = 4.184 J/g C )

Answers:
[ a) q = – 3,132.35 = –3.1 x 103 J = –3.1 kJ, exothermic process b) ∆H = – 63 kJ/mol ]

I get a) but how do I find b)?

Any help would be greatly appreciated!
Thanks in advance!

[cliverlong]

Answers:
[ a) q = – 3,132.35 = –3.1 x 103 J = –3.1 kJ, exothermic process b) ∆H = – 63 kJ/mol ]

I get a) but how do I find b)?

Any help would be greatly appreciated!
Thanks in advance!

Look at the units in the solutions

For part a) kJ

For part b) kJ/mol

So part b) tells you you need to convert the data you have, volumes and concentrations, into moles, then do your calculations.

Clive

[s3a]

I get that part a) is kJ and that part b) is kJ/mol. What I don't get is how I am supposed to find how many moles of the solution there is since the final solution is a mixture of two different solutions (HCl and NaOH).

[sjb]

How many moles of product do you get after reaction?

[s3a]

How do I know what the chemical formula for the product is? (=my problem - I think)

[MrTeo]

It's an acid - base reaction (a neutralization) so it's quite easy to understand what you get: a salt.

HA+BOH→BA+H₂O