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For the reaction Ca(OH)2(s) + H2SO4(e) → CaSO4(s) + 2H2O(e) AH° = -94.3 kJ/mol %3D How many kJ of heat are liberated or absorbed when 39.32 g of Ca(OH)2 (74.0 g/mol) are reacted with 82.94 g of H2SO4 (98.08 g/mol)? Use correct sign. Enter a number in kJ to 1 decimal place.

For the reaction Ca(OH)2(s) + H2SO4(e) → CaSO4(s) + 2H2O(e) AH° = -94.3 kJ/mol %3D How many kJ of heat are liberated or absorbed when 39.32 g of Ca(OH)2 (74.0 g/mol) are reacted with 82.94 g of H2SO4 (98.08 g/mol)? Use correct sign. Enter a number in kJ to 1 decimal place.

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter12: Thermodynamic Processes And Thermochemistry
Section: Chapter Questions
Problem 14P
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For the reaction Ca(OH)2(s) + H2SO4(e) → CaSO4(s) + 2H20(e) AH° = -94.3 kJ/mol %3D How many kJ of heat are liberated or absorbed when 39.32 g of Ca(OH), (74.0 g/mol) are reacted with 82.94 g of H,SO4 (98.08 g/mol)? Use correct sign. Enter a number in kJ to 1 decimal place.
Transcribed Image Text:For the reaction Ca(OH)2(s) + H2SO4(e) → CaSO4(s) + 2H20(e) AH° = -94.3 kJ/mol %3D How many kJ of heat are liberated or absorbed when 39.32 g of Ca(OH), (74.0 g/mol) are reacted with 82.94 g of H,SO4 (98.08 g/mol)? Use correct sign. Enter a number in kJ to 1 decimal place.
Expert Solution
Step 1

The reaction taking place is given as,

Chemistry homework question answer, step 1, image 1

Given : Mass of Ca(OH)2 taken = 39.32 g

And mass of H2SO4 taken = 82.94 g

Since mass = moles X molar mass

=> 39.32 = moles of Ca(OH)2 taken X 74.0 

=> Moles of Ca(OH)2 taken = 0.53135 mol approx.

And 82.94 = moles of H2SO4 taken X 98.08 

=> Moles of H2SO4 taken = 0.8456 mol approx.

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