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

Question

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

anonymous · Answer

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