Question

1. How many mL of H₂O₂ (l) are needed to make 8.00 L of oxygen gas according to the following balanced equation at 25 degree centigrade and 1.00 atm? The density of H₂O₂

liquid is 1.45 g/ml. Pressure is 1.05 atm and Temp is 298 K. 2H₂O₂(l) → O₂(g) + 2H₂O(l)

2. What is the mole fraction of Argon in a mixture of Ar, Ne and N₂ in a 2.70 L flask, when the partial pressures of the gases are: 0.215 atm Ar ; 0.582 atm Ne and 0.203 atm N₂? Temperature is 25 degrees C.

3. What mass of KClO₃ must be decomposed to produce 126 L of oxygen gas at 133°C and 0.880 atm? 2KClO₃(s) → 2KCl(s) + 3O₂(g)