Answer:
2.79g
Explanation:
First let us obtain the number of mole of O2 produced at 1atm and 25°C. This is illustrated below:
V (volume) = 1L
P (pressure) = 1 atm
T (temperature) = 25°C = 25 + 273 = 298K
R (gas constant) = 0.082atm.L/Kmol
n (number of mole) =?
Using the ideal gas equation PV = nRT, the number of mole can be obtained as follow:
PV = nRT
n = PV /RT
n = 1x1/(0.082x298)
n = 0.041mole
Therefore the number of mole of O2 produced is 0.041mole.
Now let us generate a balanced equation for the decomposition of Hydrogen peroxide (H2O2) to produce oxygen(O2). This is shown below:
2H2O2 —> 2H2O + O2
From the equation,
2 moles of hydrogen peroxide (H2O2) produced 1 mole of oxygen(O2).
Therefore, Xmol of Hydrogen peroxide (H2O2) will produce 0.041mole of oxygen(O2) i.e
Xmol of Hydrogen peroxide (H2O2) = 0.041 x 2 = 0.082 mole.
Now let us calculate the mass of H2O2 in 0.082 mole of H2O2. This is shown below:
Molar Mass of H2O2 = (2x1) + (16x2) = 2 + 32 = 34g/mol
Number of mole of H2O2 = 0.082 mole
Mass of H2O2 =?
Mass = number of mole x molar Mass
Mass of H2O2 = 0.082 x 34
Mass of H2O2 = 2.79g
Therefore, 2.79g of Hydrogen peroxide (H2O2) is used in the reaction
