Write the balanced chemical equation as
2 NH2CH2CO2H + 3 O2 -----------> NH2CONH2 + 3 CO2 + 3 H2O
As per the stoichiometric equation,
2 moles glycine = 3 moles CO2.
The atomic masses are
H: 1.008 g/mol.
C: 12.011 g/mol.
N: 14.007 g/mol.
O: 15.999 g/mol.
Molar mass of glycine, NH2CH2CO2H = (1*14.007 + 5*1.008 + 2*12.011 + 2*15.999) g/mol
= 75.067 g/mol.
Mass of glycine = 1.0 µg
= (1.0 µg)*(1 g)/(1.0*106 µg)
= 1.0*10-6 g.
Mol(s) glycine corresponding to 1.0 µg glycine = (1.0*10-6 g)/(75.067 g/mol)
= 1.332*10-8 mol.
Mol(s) CO2 corresponding to 1.0 µg glycine = (1.332*10-8 mol glycine)*(3 mols CO2)/(2 mols glycine)
= 1.998*10-8 mol.
Assume the liberated CO2 to behave as an ideal gas.
Pressure of the gas = 1.00 atm.
Temperature of the gas = 37ºC = (37 + 273) K = 310 K.
Use the ideal gas law to determine the volume of CO2 liberated.
PV = nRT
where n denotes the number of moles of the gas.
Therefore,
V = nRT/P
Plug in values and get
V = (1.998*10-8 mol)*(0.082 L-atm/mol.K)*(310 K)/(1.00 atm)
= 5.0789*10-7 L
= (5.0789*10-7 L)*(1.0*106 µL)/(1 L)
= 0.50789 µL
≈ 0.51 µL.
The volume of CO2 gas evolved per microgram of glycine oxidized = 0.51 µL (ans).
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