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A quantity of 4.00 x 10^2 mL of 0.600 M HNO3 is mixed with 4.00 x 10^2 mL of 0.300 M Ba(OH)2 in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of both solutions is the same at 18.46 degrees C. What is the final temperature of the solution? (Use the result in Example 6.8 for your calculation).

Results for previous example: qrxn = -2.81 KJ.

qrxn + qsoln = 0

qrxn = -qsoln

therefore, qsoln = 2.81

qsoln = ms(deltaT)

2.81 = (400 g + 400 g)(4.184 KJ/g * degrees C)(x - 18.46 degrees C)

x = [2.81/(800 g)(4.184 KJ/g * degrees C)] + 18.46 degrees C

=18.46 degrees C?

Can anybody please show me where I'm going wrong?

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# Calorimetry final temp homework help

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