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
