I'm not asking for the answer per say but does anyone know how to do this?
Calculate qsystem and qsurroundings
Calculate the qsystem and qsurroundings for the reaction and then state whether the reaction is endothermic or exothermic.
Recall that: 51.9 mL of 2.466 M HCl and 47.8 mL of 2.446 M NaOH were added together. The average temperature of the acid and base before they were added together was 22.4 oC. The products of the reaction were a salt and water. The heat capacity of the calorimeter is 1.0 X 101 J/oC. The specific heat of water is 4.184 J/(g*oC). The density of the solution can be assumed to be 1.0 g/mL.
Things I found:
Final temperature = 40.3 degrees.
mol NaOH = .1178748 mol (limiting)
mol HCl = .1229854 mol
How do you set this up?
Calculate qsystem and qsurroundings
Calculate the qsystem and qsurroundings for the reaction and then state whether the reaction is endothermic or exothermic.
Recall that: 51.9 mL of 2.466 M HCl and 47.8 mL of 2.446 M NaOH were added together. The average temperature of the acid and base before they were added together was 22.4 oC. The products of the reaction were a salt and water. The heat capacity of the calorimeter is 1.0 X 101 J/oC. The specific heat of water is 4.184 J/(g*oC). The density of the solution can be assumed to be 1.0 g/mL.
Things I found:
Final temperature = 40.3 degrees.
mol NaOH = .1178748 mol (limiting)
mol HCl = .1229854 mol
How do you set this up?
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If the temperature went up it is automatically exothermic. The surroundings is the water I will assume, so the q of the surroundings is just Q = m x c x delta t, m = (51.9 + 47.8), c = 4.184 J/(goC) and the delta t = (40.3 - 22.4)
Once you find that you should just need to divide the answer by the number of moles of NaOH or HCl to find the q of the system.
Once you find that you should just need to divide the answer by the number of moles of NaOH or HCl to find the q of the system.