When 100. mL of 1.00 M Ba(NO3)2 solution is mixed with 100. mL of 1.00 M Na₂SO4 (both solutions initially at 25.0°C) in a calorimeter, a white solid forms and the temperature of the mixture increases to 28.1°C. Assuming that the calorimeter absorbs only a negligible quantity of heat, that the specific heat capacity of the solution is 4.18 J/g.°C, and that the density of the final solution is 1.0 g/mL, calculate the enthalpy change per mole of solid that was formed. Ba(NO3)2 (aq) + Na₂SO4 (aq) → BaSO4 (s) + 2 NaNO3(aq) 2.59 kJ/mol -2.59 kJ/mol 25.9 kJ/mol -25.9 kJ/mol none of the above

When 100. mL of 1.00 M Ba(NO3)2 solution is mixed with 100. mL of 1.00 M Na₂SO4 (both solutions initially at 25.0°C) in a calorimeter, a white solid forms and the temperature of the mixture increases to 28.1°C. Assuming that the calorimeter absorbs only a negligible quantity of heat, that the specific heat capacity of the solution is 4.18 J/g.°C, and that the density of the final solution is 1.0 g/mL, calculate the enthalpy change per mole of solid that was formed. Ba(NO3)2 (aq) + Na₂SO4 (aq) → BaSO4 (s) + 2 NaNO3(aq) 2.59 kJ/mol -2.59 kJ/mol 25.9 kJ/mol -25.9 kJ/mol none of the above

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 100AE

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Question

When 100. mL of 1.00 M Ba(NO3)2 solution is mixed with 100. mL of 1.00 M Na₂SO4 (both
solutions initially at 25.0°C) in a calorimeter, a white solid forms and the temperature of the
mixture increases to 28.1°C. Assuming that the calorimeter absorbs only a negligible quantity
of heat, that the specific heat capacity of the solution is 4.18 J/g °C, and that the density of
the final solution is 1.0 g/mL, calculate the enthalpy change per mole of solid that was
formed.
Ba(NO3)2 (aq) + Na₂SO4 (aq) → BaSO4 (s) + 2 NaNO3(aq)
2.59 kJ/mol
-2.59 kJ/mol
25.9 kJ/mol
-25.9 kJ/mol
none of the above

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