Answer:
a) PN₂ = 0.733 atm
PO₂ = 0.150 atm
PCO₂ = 0.036 atm
Pwater = 0.061 atm
b) 6.44x10⁻⁴ mol
c) 0.02 g
Explanation:
a) By the Dalton's Law, in a gas mixture, the total pressure is the sum of the partial pressures, and the partial pressure is the molar fraction of the gas multiplied by the total pressure.
PN₂ = 0.748*0.980 =0.733 atm
PO₂ = 0.153*0.980 = 0.150 atm
PCO₂ = 0.037*0.980 = 0.036 atm
Pwater = 0.062*0.980 = 0.061 atm
b) The number of moles of CO₂ can be calculated by the ideal gas law:
PV = nRT, where P is the pressure, V is the volume (0.455 L), n is the number of moles, R is the gas constant (0.082 atm.L/mol.K), and T is the temperature (37°C + 273 = 310 K).
0.036*0.455 = 0.082*310*n
25.42n = 0.01638
n = 6.44x10⁻⁴ mol
c) For the combustion reaction of glucose:
C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O
So, the stoichiometry is:
1 mol of glucose ------- 6 moles of CO₂
x ------- 6.44x10⁻⁴ mol of CO₂
By a simple direct three rule:
6x = 6.44x10⁻⁴
x = 1.073x10⁻⁴mol of glucose
Glucose has a molar mass equal to 180 g/mol, and its mass is the molar mass multiplied by the number of moles:
m = 180x1.073x10⁻⁴
m = 0.02 g
