**Answer:**

(a) To calculate the oxygen gas produced in litters at STP when the compound undergoes complete decomposition. First note the equation at decomposition below

2H2O2(aq) → 2H2O(l) + O2(g)

Then

(3.0 g/100 ml)(10 ml) = 0.3 g H2O2

divide by Mass of H2O2 which is 34 g/mole,

0.3/34 = 0.00882353

this will arise to 8.8 x 10-3 molesH2O2

then multiply the moles H2O2 by: (1 mole O2/2 mole H2O2)= 4.4 x 10-3moles O2

To calculate the volume (in L) of Oxygen 02, we have to use the ideal gas equation:

VO2 = nO2RT/P;

n = 4.4 x10-3moles, P = 1 atm, R - 0.0826 L-atm/mol-K andT = 273K

V02 = 99.22 X 10∧-3

(b) divide volume of O2 from (a) by 10 ml (0.010L - initialvolume of H2O2)

9.92 X10∧-3

**Explanation:**

a) To calculate the oxygen gas produced in litters at STP when the compound undergoes complete decomposition. First note the equation at decomposition below

2H2O2(aq) → 2H2O(l) + O2(g)

Then

(3.0 g/100 ml)(10 ml) = 0.3 g H2O2

divide by Mass of H2O2 which is 34 g/mole,

0.3/34 = 0.00882353

this will arise to 8.8 x 10-3 molesH2O2

then multiply the moles H2O2 by: (1 mole O2/2 mole H2O2)= 4.4 x 10-3moles O2

To calculate the volume (in L) of Oxygen 02, we have to use the ideal gas equation:

VO2 = nO2RT/P;

n = 4.4 x10-3moles, P = 1 atm, R - 0.0826 L-atm/mol-K andT = 273K

V02 = 99.22 X 10∧-3

(b) divide volume of O2 from (a) by 10 ml (0.010L - initialvolume of H2O2)

9.92 X10∧-3