Question

In a constant-pressure calorimeter of negligible heat capacity, 25 mL of 1.00 M CaCl2 is mixed with 25 mL of 2.00 M KF, resulting in solid CaF2 precipitating out of the solution. During this process, the temperature of the water rises from 25.0°C to 26.7°C. Assume the specific heat capacity of the solution is 4.184 J/°C•g and the density of the solution is 1.00 g/mL. Calculate the enthalpy of precipitation in kJ per mole of CaF2 precipitated.

Answer #1

5. When 1.00L of a 1.00 M Ba(NO3)2 solution at 25.0oC is mixed
with 1.00 L of a 1.00 M Na2SO4 solution at 25.0oC in a calorimeter,
the white solid, BaSO4 forms and the temperature of the mixture
increases to 28.1oC. Assuming that the calorimeter absorbs only a
negligible quantity of heat, that the specific heat capacity of the
solution is 4.18 J/oC g and that the density of the final solution
is 1.0 g/mL, calculate the enthalpy change per...

When 100 mL of Ba(NO3)2 solution at 25 degrees Celsius is
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calorimeter absorbs only a negligible quantity of heat and the
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Celsius, and that the density of the final solution is 1.0 g/mL,
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When an excess of Zn is added to 125mL of 0.150M CuSO4(aq) in a
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In a constant-pressure calorimeter, 60.0 mL of 0.780 M H2SO4 was
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of the individual volumes.
I am stuck on...

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