Respuesta :
The partial pressure contributed to the overall pressure is proportional to the number of moles of gas particles. Both Neon and Argon are noble gases so there's just 1 atom per molecule. So let's determine how many moles of each we have:
Atomic weight neon = 20.1797
Atomic weight argon = 39.948
Moles neon = 10.0 g / 20.1797 g/mol = 0.495547506 mol
Moles argon = 10.0 g / 39.948 g/mol = 0.250325423 mol
So there's a total of 0.495547506 + 0.250325423 = 0.745872929 moles of gas particles. And for neon, it contributes 0.495547506/0.745872929 = 0.664385965 = 66.4385965% of them, so it contributes 66.4385965% of the total pressure. Which is 66.4385965% * 1.6 atm = 1.063017544 atm.
Rounding to 3 significant figures gives 1.06 atm, or 66.4% of the total pressure.
Atomic weight neon = 20.1797
Atomic weight argon = 39.948
Moles neon = 10.0 g / 20.1797 g/mol = 0.495547506 mol
Moles argon = 10.0 g / 39.948 g/mol = 0.250325423 mol
So there's a total of 0.495547506 + 0.250325423 = 0.745872929 moles of gas particles. And for neon, it contributes 0.495547506/0.745872929 = 0.664385965 = 66.4385965% of them, so it contributes 66.4385965% of the total pressure. Which is 66.4385965% * 1.6 atm = 1.063017544 atm.
Rounding to 3 significant figures gives 1.06 atm, or 66.4% of the total pressure.
The partial pressure of Ne is [tex]\boxed{1.063{\text{ atm}}}[/tex].
Further Explanation:
Dalton’s law:
This law states that partial pressure of any gas is calculated by the multiplication of mole fraction and the total pressure of gas mixture.
The expression for partial pressure of a particular gas is,
[tex]{P_{{\text{gas}}}} = {X_{{\text{gas}}}} \cdot {P_{{\text{total}}}}[/tex] …… (1)
Where,
[tex]{P_{\text{gas}[/tex] is the partial pressure of the gas.
[tex]{P_{{\text{total}}[/tex] is the total pressure of the mixture.
[tex]{X_{{\text{gas}}}[/tex] is the mole fraction of gas.
The formula to calculate moles of component is as follows:
[tex]{\text{Moles of component}} = \dfrac{{{\text{Mass of component}}}}{{{\text{Molar mass of component}}}}[/tex] …… (2)
Substitute 10.0 g for mass of component and 20.179 g/mol for molar mass of component in equation (2) to calculate moles of Ne.
[tex]\begin{aligned}{\text{Moles of Ne}} &= \frac{{{\text{10}}{\text{.0 g}}}}{{{\text{20}}{\text{.179 g/mol}}}} \\ &= 0.4956{\text{ mol}} \\\end{aligned}[/tex]
Substitute 10.0 g for mass of component and 39.948 g/mol for molar mass of component in equation (2) to calculate moles of Ar.
[tex]\begin{aligned}{\text{Moles of Ar}} &= \frac{{{\text{10}}{\text{.0 g}}}}{{{\text{39}}{\text{.948 g/mol}}}} \\&= 0.2503{\text{ mol}} \\ \end{aligned}[/tex]
Total number of moles can be calculated as follows:
[tex]\begin{aligned}{\text{Total number of moles}} &= \left( {0.4956 + 0.2503} \right){\text{ mol}} \\ &= 0.7459{\text{ mol}} \\\end{aligned}[/tex]
The formula to calculate mole fraction of Ne is as follows:
[tex]{\text{Mole fraction of Ne}} = \dfrac{{{\text{Moles of Ne}}}}{{{\text{Total number of moles}}}}[/tex] …… (3)
Substitute 0.4956 mol for moles of Ne and 0.7459 mol for total number of moles in equation (3).
[tex]\begin{aligned}{\text{Mole fraction of Ne}} &= \frac{{{\text{0}}{\text{.4956 mol}}}}{{{\text{0}}{\text{.7459 mol}}}} \\&= 0.6644 \\\end{aligned}[/tex]
Substitute 0.6644 for [tex]{X_{{\text{gas}}}}[/tex] and 1.6 atm for [tex]{P_{{\text{total}}}}[/tex] in equation (1) to calculate partial pressure of Ne.
[tex]\begin{aligned}{P_{{\text{Ne}}}} &= \left( {0.6644} \right)\left( {1.6{\text{ atm}}} \right) \\&= 1.063{\text{ atm}} \\\end{aligned}[/tex]
Learn more:
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Answer details:
Grade: Middle School
Subject: Chemistry
Chapter: Gases and the kinetic-molecular theory
Keywords: partial pressure, mole fraction, Ne, Ar, moles, molar mass, mass, 1.063 atm, 1.6 atm, 0.6644, mole fraction of Ne.
