Explore BrainMass

Explore BrainMass

    Thermodynamic Data and Standard Enthalpy of Decomposition

    This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!

    Use thermodynamic data to calculate the standard enthalpy of decomposition of liquid hydrogen peroxide into water and oxygen gas: H2O2(l)-->H2O(g) + 1/2 O2(g).
    Calculate the energy released by the decomposition of 1.0 g of 90% hydrogen peroxide solution. Molar mass of hydrogen peroxide = 34.0 g/mol. Estimate the final temperature of the product gases of the decomposition. Assume that the constant-volume heat capacities of water and oxygen are respectively 35, and 25 J/mol/K.
    enthalpy of H2O2(l) = -187.8 kJ/mol
    enthalpy of H20(g) = -241.8 kJ/mol
    enthalpy of O2(g) = 0 kJ/mol

    © BrainMass Inc. brainmass.com March 4, 2021, 5:50 pm ad1c9bdddf
    https://brainmass.com/chemistry/energetics-and-thermodynamics/thermodynamic-data-and-standard-enthalpy-of-decomposition-13481

    Solution Preview

    Since mass of H2O2 = 1.0*90/100 = 0.9 gm
    The number of moles of H2O2 = 0.9/34 = 0.02647 mol
    This is because 1 mole of H2O2 gives out 1 mole of H2O and 1/2 mole of O2.
    Hence, 0.02647 mol of H2O2 will produce 0.02647 mol ...

    Solution Summary

    The solution uses thermodynamic data to find the standard enthalpy of decomposition of liquid hydrogen peroxide into water and oxygen gas. The solution also calculates the energy released and the final temperature from the decomposition.

    $2.49

    ADVERTISEMENT