6485.2 J is right and it is lost BUT by the reaction and not the calorimeter. Since the calorimeter changed T from 22.5 UP TO 34.9 that means the calorimeter gained heat and that means the reaction is exothermic (it released the heat which the calorimeter absorbed).
b. How many mols reacted. That's M x L = 1.86 x 0.0625 = 0.11625
So rxn released 6485.2 J/0.11625 mol = ? J/mol
c. The reaction is exothermic as discussed in part a.
d. d is ok.
The reaction between sodium hydroxide and hydrobromic acid is represented in the equation below:
OH- + H+ -> H2O
A 62.5 mL sample of 1.86 M NaOH at 22.5 deg Celsius was mixed with 62.5 mL sample of 1.86 M of HBr at 22.5 deg Celsius in a coffee cup calorimeter. The temperature increased from 22.5-34.9 degrees. Assume that the volumes are additive, that the specific heat of the solution is the same as that of water, and that the density of the solution is 1.00g/mL
a. Find the amount of heat lost or gained by the calorimeter
b. Find the heat of reaction, when one mole of sodium hydroxide, NaOH, reacts with one mole of hyrdobromic acid in water.
c. Is the reaction endothermic or exothermic?
d. Was energy conserved in the process?
for a) I got 6485.2 joules lost
for b), I don't know how to do this so an explanation would be great:)
for c) I got endothermic
for d) I said that energy was conserved
are my answers correct? im trying to study for a test and I would like to make sure that I am doing this right:)
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