I don't agree with either answer.
q from H2O = 200*4.184(5.98) = ?
q from calorimeter = 100*5.98
Total q for 0.1 mols is the sum of the two above.
Then q/mol = sum/0.1 = ? I get about 55 kJ/mol
You can mix 100.mL of 1.0 M HCl with 100 mL of 1.0 NaOH, both at 25 degree Celcius. The temperature of your calorimeter rises by 5.98 degree C, and its heat capacity is 100 J/degre C. How much energy is released per mol of H2O formed?
My answer: 6x10^6 J per mol H2O
I think we are trying to find the total change in energy... so that would be change in energy of solution + change in energy of the beaker....
Bobpursley's answer:
Ok, you will make .1 mole of H2O
you have 200ml of water heating 5.99C
Heat released=mass*c*deltaTemp
=200*100J/C*5.98C
heat released per mole
= heatreleased/.1 J/mole
Unless I made an error, your answer is wrong.
1 answer
0 answers