Hydrogen peroxide decomposes into water and oxygen - H2O2 → H2O + O2 Use the balanced equation above to calculate the following: a. What mass of oxygen is produced when 1.840 mol of H2O2 decomposes?

b. How many molecules of oxygen is this?

c. How many Liters of oxygen, measured at STP, is this? ​

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

c. is the answer

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