1)
The balanced equation is
2 CO + O2 -------> 2 CO2
PV = nRT
P = pressure = 1 atm
V = volume = 26.7 L
n = number of moles
R = Gas constant
T = temperature = 0 + 273 = 273 K
1 * 38.4 = n * 0.0821*273
38.4 = n * 22.4
n = 38.4 / 22.4 = 1.71 mole
From the balanced equation we can say that
1 mole of O2 requires 2 mole of CO so
1.71 mole of O2 will require
= 1.71 mole of O2 *(2 mole of CO / 1 mole of O2)
= 3.42 mole of CO
Therefore, the number of moles of CO = 3.42 mole
2) 2 H2O2 -----> 2 H2O + O2
PV = nRT
1 * 26.7 = n * 0.0821 * 273
26.7 = n * 22.4
n = 26.7 / 22.4 = 1.19 mol
number of moles of O2 = 1.19 mol
From the balanced equation we can say that
1 mole of O2 requires 2 mole of H2O2 so
1.19 mole of O2 will require
= 1.19 mole of O2 *(2 mole of H2O2 / 1 mole of O2)
= 2.38 mole of H2O2
mass of 1 mole of H2O2 = 34.0147 g
so the mass of 2.38 mole of H2O2 = 81.0 g
Therefore, the mass of H2O2 required would be 81.0 g
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