The decomposition of one mole of hydrogen peroxide, H2O2(s), into water and oxygen gas, at constant pressure releases 98 kJ of heat.   Write a balanced thermochemical equation for the reaction. Which has the higher enthalpy under these conditions, the reactants or the products? How many kJ of energy would be released if 68 grams of hydrogen peroxide are decomposed.

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The decomposition of one mole of hydrogen peroxide, H2O2(s), into water and oxygen gas, at constant pressure releases 98 kJ of heat.

 

  1. Write a balanced thermochemical equation for the reaction.



  1. Which has the higher enthalpy under these conditions, the reactants or the products?



  1. How many kJ of energy would be released if 68 grams of hydrogen peroxide are decomposed.




  1. Would the enthalpy change for the reaction be greater or less if water vapor formed rather than liquid water?




  1. Write a balanced thermochemical equation for the reverse of the reaction you wrote in (a) above.





  1. For the reaction in (e) how many kJ of energy would be required to make 17 grams of hydrogen peroxide?
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