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1
1.) The specific heat of a solution is 4.18 J/(grams x degrees Celsius) and its density is 1.02 g/mL. The solution is formed by combining 20.0 mL of solution A with 30.0 mL of solution B, both initially at 21.4 degrees Celsius. The final temperature is 25.3 degrees Celsius. Calculate the heat of reaction. assuming no heat is lost to the calorimeter.
2.) In the problem above, the calorimeter used has a heat capacity of 8.20 J/degrees Celsius. If you include a correction for the heat absorbed by the calorimeter, what is the heat of reaction.
Expert Solution
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1) The specific heat of a solution is 4.18 J/(g 0C) and its density is 1.02 g/mL. The solution is formed by combining 20.0 mL of solution A with 30.0 mL of solution B, both initially at 21.40C. The final temperature is 25.30C. Calculate the heat of reaction assuming no heat is lost to the calorimeter.
qrxn= -qca -qsoln = -(Ccal + msoln ssoln )(Tf - Ti )
Since qcal = 0 here, qrxn= -(msoln ssoln)(Tf - Ti)
For solution A, qA = -(1.02*20*4.18)(25.3 - 21.4) = -332.56 J
For solution B, qB = -(1.02*30*4.18)(25.3 - 21.4) = -498.84 J
Total heat of solution = -332.56 J - 498.84 J = -831.4 J
2) In the problem above, the calorimeter used has a heat capacity of 8.20 J/ 0C. If you include a correction for the heat absorbed by the calorimeter, what is the heat of reaction?
Heat of reaction = -8.20*(25.3 - 21.4) - 831.4 = -863.38 J
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