Hydrogen peroxide with concentration of
3.0percent ( 3.0 g of h202 in 100 ml of solution) is sold
indrugstorese ofo use as an antiseptic. for a 10 ml 3.0 percenet
h202solution, calculate (a) the oxygen gas produce in litters at
stpwhen the compount undergoes complete decompostion and (b)
thteratio of the volume of 02 collected to the intial volume of
theh2o2 solution.

(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

the correct answer would be d. hope this !

the cold front replaces the warmer air at the ground level changing the wind to be breezy and denser.there is also an immediate drop in the temperature.