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A 100.0-mL sample of 1.00 M NaOH is mixed with 50.0 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup calorimeter fitted with a lid through which a thermometer passes.  The acid-base reaction is as follows:                        2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(ℓ) The temperature of each solution before mixing is 22.3 °C.  After mixing, the temperature of the solution mixture reaches a maximum temperature of 31.4 °C.  Assume the density of the solution mixture is 1.00 g/mL, its specific heat is 4.18 J/g⋅°C, and no heat is lost to the surroundings. Calculate the enthalpy change, in kJ, per mole of H2SO4 in the reaction. +85.6 kJ/mol ‒85.6 kJ/mol +5.71  kJ/mol ‒5.71 kJ/mol ‒114 kJ/mol

A 100.0-mL sample of 1.00 M NaOH is mixed with 50.0 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup calorimeter fitted with a lid through which a thermometer passes.  The acid-base reaction is as follows:                        2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(ℓ) The temperature of each solution before mixing is 22.3 °C.  After mixing, the temperature of the solution mixture reaches a maximum temperature of 31.4 °C.  Assume the density of the solution mixture is 1.00 g/mL, its specific heat is 4.18 J/g⋅°C, and no heat is lost to the surroundings. Calculate the enthalpy change, in kJ, per mole of H2SO4 in the reaction. +85.6 kJ/mol ‒85.6 kJ/mol +5.71  kJ/mol ‒5.71 kJ/mol ‒114 kJ/mol

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 100.0-mL sample of 1.00 M NaOH is mixed with 50.0 mL of 1.00 M H2SO4 in a large Styrofoam coffee cup calorimeter fitted with a lid through which a thermometer passes.  The acid-base reaction is as follows:

                       2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(ℓ)

The temperature of each solution before mixing is 22.3 °C.  After mixing, the temperature of the solution mixture reaches a maximum temperature of 31.4 °C.  Assume the density of the solution mixture is 1.00 g/mL, its specific heat is 4.18 J/g⋅°C, and no heat is lost to the surroundings. Calculate the enthalpy change, in kJ, per mole of H2SO4 in the reaction.

+85.6 kJ/mol

‒85.6 kJ/mol

+5.71  kJ/mol

‒5.71 kJ/mol

‒114 kJ/mol

 
 
 

 

 

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