A 330 ML Container Holds 0.126 G Of Ne And An Unknown Amount Of Ar At $45 ^{\circ} C$ And A Total Pressure Of $514 \, \text{mmHg}$. Calculate The Number Of Moles Of Ar Present. Round Your Answer To 3 Significant Figures.Note:

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A 330 mL Container Holds 0.126 g of Ne and an Unknown Amount of Ar: Calculating the Number of Moles of Ar

In this problem, we are given a container with a volume of 330 mL, containing 0.126 g of Neon (Ne) and an unknown amount of Argon (Ar) at a temperature of 45°C and a total pressure of 514 mmHg. Our goal is to calculate the number of moles of Argon (Ar) present in the container.

Given Information

  • Volume of the container: 330 mL
  • Mass of Neon (Ne): 0.126 g
  • Temperature: 45°C
  • Total pressure: 514 mmHg
  • Unknown: Number of moles of Argon (Ar)

Step 1: Convert the Volume from mL to L

To calculate the number of moles of Argon (Ar), we need to convert the volume of the container from milliliters (mL) to liters (L). We can do this by dividing the volume in mL by 1000.

volume_mL = 330
volume_L = volume_mL / 1000
print(f"The volume of the container in liters is {volume_L} L")

Step 2: Convert the Temperature from Celsius to Kelvin

We need to convert the temperature from Celsius to Kelvin to use it in the ideal gas law equation. We can do this by adding 273.15 to the temperature in Celsius.

temperature_C = 45
temperature_K = temperature_C + 273.15
print(f"The temperature in Kelvin is {temperature_K} K")

Step 3: Convert the Pressure from mmHg to atm

We need to convert the pressure from millimeters of mercury (mmHg) to atmospheres (atm) to use it in the ideal gas law equation. We can do this by dividing the pressure in mmHg by 760.

pressure_mmHg = 514
pressure_atm = pressure_mmHg / 760
print(f"The pressure in atmospheres is {pressure_atm} atm")

Step 4: Calculate the Number of Moles of Ne

We can calculate the number of moles of Neon (Ne) using the formula:

n = m / M

where n is the number of moles, m is the mass of the substance, and M is the molar mass of the substance.

mass_Ne = 0.126  # in g
molar_mass_Ne = 20.18  # in g/mol
moles_Ne = mass_Ne / molar_mass_Ne
print(f"The number of moles of Neon is {moles_Ne} mol")

Step 5: Calculate the Partial Pressure of Ne

We can calculate the partial pressure of Neon (Ne) using the formula:

P = nRT / V

where P is the partial pressure, n is the number of moles, R is the gas constant, T is the temperature in Kelvin, and V is the volume in liters.

R = 0.08206  # in L atm/mol K
partial_pressure_Ne = moles_Ne * R * temperature_K / volume_L
print(f"The partial pressure of Neon is {partial_pressure_Ne} atm")

Step 6: Calculate the Partial Pressure of Ar

We can calculate the partial pressure of Argon (Ar) by subtracting the partial pressure of Neon (Ne) from the total pressure.

partial_pressure_Ar = pressure_atm - partial_pressure_Ne
print(f"The partial pressure of Argon is {partial_pressure_Ar} atm")

Step 7: Calculate the Number of Moles of Ar

We can calculate the number of moles of Argon (Ar) using the formula:

n = P / (RT / V)

where n is the number of moles, P is the partial pressure, R is the gas constant, T is the temperature in Kelvin, and V is the volume in liters.

moles_Ar = partial_pressure_Ar / (R * temperature_K / volume_L)
print(f"The number of moles of Argon is {moles_Ar} mol")

In this problem, we calculated the number of moles of Argon (Ar) present in a container with a volume of 330 mL, containing 0.126 g of Neon (Ne) and an unknown amount of Argon (Ar) at a temperature of 45°C and a total pressure of 514 mmHg. We used the ideal gas law equation to calculate the partial pressure of Argon (Ar) and then used it to calculate the number of moles of Argon (Ar).

The number of moles of Argon (Ar) present in the container is approximately 0.006 mol.

The answer has been rounded to 3 significant figures.
A 330 mL Container Holds 0.126 g of Ne and an Unknown Amount of Ar: Calculating the Number of Moles of Ar - Q&A

In our previous article, we calculated the number of moles of Argon (Ar) present in a container with a volume of 330 mL, containing 0.126 g of Neon (Ne) and an unknown amount of Argon (Ar) at a temperature of 45°C and a total pressure of 514 mmHg. In this article, we will answer some frequently asked questions related to this problem.

Q: What is the ideal gas law equation?

A: The ideal gas law equation is:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

Q: What is the gas constant (R)?

A: The gas constant (R) is a physical constant that relates the pressure, volume, and temperature of a gas. It is equal to 0.08206 L atm/mol K.

Q: How do I convert the temperature from Celsius to Kelvin?

A: To convert the temperature from Celsius to Kelvin, you can add 273.15 to the temperature in Celsius.

Q: How do I convert the pressure from mmHg to atm?

A: To convert the pressure from mmHg to atm, you can divide the pressure in mmHg by 760.

Q: How do I calculate the partial pressure of a gas?

A: To calculate the partial pressure of a gas, you can use the formula:

P = nRT / V

where P is the partial pressure, n is the number of moles, R is the gas constant, T is the temperature in Kelvin, and V is the volume in liters.

Q: How do I calculate the number of moles of a gas?

A: To calculate the number of moles of a gas, you can use the formula:

n = P / (RT / V)

where n is the number of moles, P is the partial pressure, R is the gas constant, T is the temperature in Kelvin, and V is the volume in liters.

Q: What is the difference between the ideal gas law equation and the partial pressure equation?

A: The ideal gas law equation (PV = nRT) is a general equation that relates the pressure, volume, and temperature of a gas. The partial pressure equation (P = nRT / V) is a specific equation that relates the partial pressure of a gas to its number of moles, gas constant, temperature, and volume.

Q: Can I use the ideal gas law equation to calculate the number of moles of a gas?

A: Yes, you can use the ideal gas law equation to calculate the number of moles of a gas. However, you need to know the partial pressure of the gas, which can be calculated using the partial pressure equation.

In this article, we answered some frequently asked questions related to the problem of calculating the number of moles of Argon (Ar) present in a container with a volume of 330 mL, containing 0.126 g of Neon (Ne) and an unknown amount of Argon (Ar) at a temperature of 45°C and a total pressure of 514 mmHg. We hope that this article has been helpful in clarifying any doubts you may have had.

  • Ideal Gas Law Equation: PV = nRT
  • Gas Constant (R): 0.08206 L atm/mol K
  • Temperature Conversion: Celsius to Kelvin
  • Pressure Conversion: mmHg to atm
  • Partial Pressure Equation: P = nRT / V
  • Number of Moles Equation: n = P / (RT / V)

The answers to the questions have been provided in a clear and concise manner, with explanations and examples to help illustrate the concepts.