Answer:
The true statement is option A.
Explanation:
Using ideal gas equation:
PV = nRT
where,
P = Pressure of gas = 1 atm
V = Volume of gas = ?
n = number of moles of gas = 1 mol
R = Gas constant = 0.0821 L.atm/mol.K
T = Temperature of gas = 273.15 K
[tex]V=\frac{nRT}{P}=\frac{1 mol\times 0.0821 atm L/mol K\times 273.15 K}{1 atm}[/tex]
V = 22.42 L
This means that 1 mole of an ideal gas at STP occupies 22.42 liters of volume.
So, 1 mole of helium gas and 1 mole of oxygen gas will have same value of volume in their respective balloons at STP.
Considering the definition of STP conditions, the correct answer is option (A): The balloons will have the same volume.
The STP conditions refer to the Standard Temperature and Pressure. Pressure values at 1 atmosphere and temperature at 0 ° C are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.
Standard reference conditions are important for expressions of fluid flow and volumes of liquids and gases, which are highly dependent on temperature and pressure.
In summary, 1 mole of helium gas and 1 mole of oxygen gas will have same value of volume in their respective balloons at STP.
Then, the correct answer is option (A): The balloons will have the same volume.
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