Respuesta :
How many liters of oxygen gas were used up?
If 185 g of wax [tex]C_{22}H_{44}[/tex] burns, 13.73 L of oxygen gas is used.
An ideal gas equation is:
The macroscopic characteristics of ideal gases are related to the ideal gas law (PV = nRT). Gas is considered to be perfect if its particles (a) do not interact with one another and (b) occupy no space (have no volume).
First, determine the gas's moles using the gas law.
PV = nRT, where n is the number of moles and R is the gas constant. Next, divide.
To obtain molar mass, multiply the given mass by the number of moles.
Data provided:
P= 101kpa =0.996792 atm
V= ?
R= 0.082057338 L atm K[tex]^{1} mol^{-1}[/tex]
T=25 +273 =298 K
Moles =?
Moles = mass/molar mass = 185g/308.6
Moles =0.56
Putting value in the given equation:
PV/RT =n
0.56 = [tex]\frac{0.996792 atm XV}{0.082057338 L atm K^{1} mol^{-1} X 298}[/tex]
13.73 L =V
13.73 L of oxygen gas was used up if 185 g of [tex]C_{22}H_{44}[/tex] wax burns.
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