a 4.976 g sample of potassium sulfate is added to a coffee cup calorimeter conta

Question

a 4.976 g sample of potassium sulfate is added to a coffee cup calorimeter containing 122.6 g of distilled water at 22.43 degrees Celsius. After the sample had dissolved, the temperature was 21.11 C. What is the molar heat of solution of potassium sulfate? a 4.976 g sample of potassium sulfate is added to a coffee cup calorimeter containing 122.6 g of distilled water at 22.43 degrees Celsius. After the sample had dissolved, the temperature was 21.11 C. What is the molar heat of solution of potassium sulfate? a 4.976 g sample of potassium sulfate is added to a coffee cup calorimeter containing 122.6 g of distilled water at 22.43 degrees Celsius. After the sample had dissolved, the temperature was 21.11 C. What is the molar heat of solution of potassium sulfate?

Explanation / Answer

Heat released by water = m*C*delta T

= 122.6 g * 4.184 J/g.oC * (22.43 - 21.11) oC

= 677.1 J

This heat must be absorbed while dissolving

number of mol of K2SO4,

n = mass of K2SO4 / molar mass of K2SO4

= 4.976 g / 174.3 g/mol

= 0.0285 mol

H solution = Q / number of mol

= 677.1 J / 0.0285 mol

= 2.37*10^4 J/mol

= 23.7 KJ/mol

Answer: 23.7 KJ/mol

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