6) 2.00 grams of NaOH is added to 100.0 mL of water at 22.0 °C. After dissolving, the temperature of the solution is found to be 27.3°C. (Assume that the specific heat of the solution is 4.184 J/g°C and the density of the solution is 1.00 g/mL) a) Find the experimental value for the molar enthalpy of dissolution for NaOH. b) Write the equation for the dissolution of NaOH, including the value for AH.
6) 2.00 grams of NaOH is added to 100.0 mL of water at 22.0 °C. After dissolving, the temperature of the solution is found to be 27.3°C. (Assume that the specific heat of the solution is 4.184 J/g°C and the density of the solution is 1.00 g/mL) a) Find the experimental value for the molar enthalpy of dissolution for NaOH. b) Write the equation for the dissolution of NaOH, including the value for AH.
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Transcribed Image Text:6) 2.00 grams of NaOH is added to 100.0 mL of water at 22.0 °C. After dissolving, the temperature of the
solution is found to be 27.3°C. (Assume that the specific heat of the solution is 4.184 J/g°C and the
density of the solution is 1.00 g/mL)
a) Find the experimental value for the molar enthalpy of dissolution for NaOH.
b) Write the equation for the dissolution of NaOH, including the value for AH.
Expert Solution
Step 1
Given that, 2 g of NaOH dissolved in 100 mL of water.
The initial temperature is T1 = 22oC.
The final temperature of the solution is T2 = 27.3oC.
The specific heat of the solution is C = 4.184 J/g.oC.
The density of water is 1 g/mL.
(a) We have to calculate the molar enthalpy of dissolution of NaOH.
(b) We also have to write the dissolution equation of NaOH.
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