A gas mixture in a 1.55L at 298K container contains 10.0g Ne and 10.0g Ar. Calculate the partial pressure " in atm" of Ne and Ar in the container

Question

Create a detailed scientific illustration of a laboratory setting. On one side of the image, have a 1.55 liter transparent container holding a blend of two distinct types of gas molecules, represented by different colors, signifying Neon and Argon. The container is placed on a table, and we can see the temperature indicator reading 298K. On the other side of the image, display some weighing scales with weight readings showing 10.0g for two separate piles of different colored spheres, indicating the amount of Neon and Argon in the container. Remember, the image should not contain any text.

A gas mixture in a 1.55L at 298K container contains 10.0g Ne and 10.0g Ar. Calculate the partial pressure " in atm" of Ne and Ar in the container

Answer 1

10.0 g Ne / 20.18 g/mol = 0.496 mol

P*1.55 L = 0.496 mol * 0.08206 L*atm/mol*K * 298 K
P of Ne = 7.82 atm

10.0 g Ar / 39.948 g/mol = 0.25 mol
P*1.55 L = 0.25 mol * 0.08206 L*atm/mol*K * 298 K
P of Ar = 3.94 atm

Answer 2

Well, well, looks like we've got a gas mixture trying to figure out its pressure! Neat-o! Let's get cracking!

First things first, we need to find the moles of each gas. To do that, we divide the mass of each gas by their respective molar masses. For Ne (Neon), the molar mass is 20.18 g/mol, and for Ar (Argon), it's 39.95 g/mol.

So, for Ne: 10.0 g / 20.18 g/mol = 0.495 mol
And for Ar: 10.0 g / 39.95 g/mol = 0.250 mol

Now, we need to calculate the partial pressure of each gas. Remember, partial pressure is just the pressure of each gas if it were the only gas in the container.

To find the partial pressure, we use the ideal gas law equation: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant (0.0821 L.atm/mol.K), and T is the temperature in Kelvin.

For Ne: P_Ne = (n_Ne * R * T) / V = (0.495 mol * 0.0821 L.atm/mol.K * 298 K) / 1.55 L = 7.11 atm
For Ar: P_Ar = (n_Ar * R * T) / V = (0.250 mol * 0.0821 L.atm/mol.K * 298 K) / 1.55 L = 3.50 atm

So, the partial pressure of Ne is 7.11 atm and the partial pressure of Ar is 3.50 atm.

Voila! We've got our pressure party all figured out!

Answer 3

To calculate the partial pressures of Ne and Ar in the container, we need to consider the ideal gas law and Dalton's law of partial pressures.

1. Calculate the number of moles of Ne and Ar:
- Number of moles of Ne: n_ne = mass of Ne / molar mass of Ne
The molar mass of Ne is 20.18 g/mol.
- Number of moles of Ar: n_ar = mass of Ar / molar mass of Ar
The molar mass of Ar is 39.95 g/mol.

2. Calculate the total moles of gas in the mixture:
Total moles of gas = n_ne + n_ar

3. Calculate the mole fraction of Ne:
Mole fraction of Ne = (moles of Ne) / (total moles of gas)

4. Calculate the mole fraction of Ar:
Mole fraction of Ar = (moles of Ar) / (total moles of gas)

5. Calculate the partial pressure of Ne:
Partial pressure of Ne = (mole fraction of Ne) * (total pressure)

6. Calculate the partial pressure of Ar:
Partial pressure of Ar = (mole fraction of Ar) * (total pressure)

Now we can calculate the partial pressure of Ne and Ar in the container.

Let's begin the calculations:

1. Number of moles of Ne:
n_ne = 10.0 g / 20.18 g/mol

2. Number of moles of Ar:
n_ar = 10.0 g / 39.95 g/mol

3. Total moles of gas:
total moles of gas = n_ne + n_ar

4. Mole fraction of Ne:
mole fraction of Ne = n_ne / total moles of gas

5. Mole fraction of Ar:
mole fraction of Ar = n_ar / total moles of gas

6. Partial pressure of Ne:
partial pressure of Ne = mole fraction of Ne * total pressure

7. Partial pressure of Ar:
partial pressure of Ar = mole fraction of Ar * total pressure

Note: We need to convert the temperature to Kelvin by adding 273.15 K.

Let's calculate the partial pressures step by step.

1. Molar mass of Ne:
molar mass of Ne = 20.18 g/mol

Number of moles of Ne:
n_ne = 10.0 g / 20.18 g/mol ≈ 0.494 mol

2. Molar mass of Ar:
molar mass of Ar = 39.95 g/mol

Number of moles of Ar:
n_ar = 10.0 g / 39.95 g/mol ≈ 0.251 mol

3. Total moles of gas:
total moles of gas = n_ne + n_ar ≈ 0.494 mol + 0.251 mol ≈ 0.745 mol

4. Mole fraction of Ne:
mole fraction of Ne = n_ne / total moles of gas
= 0.494 mol / 0.745 mol ≈ 0.663

5. Mole fraction of Ar:
mole fraction of Ar = n_ar / total moles of gas
= 0.251 mol / 0.745 mol ≈ 0.337

6. Partial pressure of Ne:
partial pressure of Ne = mole fraction of Ne * total pressure

7. Partial pressure of Ar:
partial pressure of Ar = mole fraction of Ar * total pressure

Now you need to provide the total pressure in the container, and I can calculate the partial pressures of Ne and Ar.

Answer 4

To calculate the partial pressure of Ne and Ar in the container, you need to use the ideal gas law equation:

PV = nRT

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

First, we need to calculate the number of moles for each gas. To do that, we'll use the molar mass for each gas:

Molar mass of Ne = 20.18 g/mol
Molar mass of Ar = 39.95 g/mol

Number of moles for Ne:
n(Ne) = mass of Ne / molar mass of Ne
n(Ne) = 10.0 g / 20.18 g/mol

Number of moles for Ar:
n(Ar) = mass of Ar / molar mass of Ar
n(Ar) = 10.0 g / 39.95 g/mol

Next, we'll calculate the total number of moles by summing the number of moles of Ne and Ar:

Total moles = n(Ne) + n(Ar)

Now, we can calculate the partial pressure of Ne and Ar using the ideal gas law.

For Ne:
P(Ne) = (n(Ne) / Total moles) * P(total)

For Ar:
P(Ar) = (n(Ar) / Total moles) * P(total)

Since the container contains a mixture of Ne and Ar and no other gases are mentioned, the total pressure of the mixture is equal to the partial pressure of Ne plus the partial pressure of Ar:

P(total) = P(Ne) + P(Ar)

To simplify the equation further, we can rewrite the partial pressure expressions:

P(Ne) = (n(Ne) / Total moles) * P(total)
P(Ar) = (n(Ar) / Total moles) * P(total)
P(total) = P(Ne) + P(Ar)

Now, substitute the given values into the equations and calculate the partial pressures of Ne and Ar in the container.

Note: To get the pressure in atm, you need to convert the pressure to the appropriate unit using the appropriate value for R.

R = 0.0821 L*atm/(mol*K)

After substituting the values and calculating, you will obtain the partial pressures of Ne and Ar in atm.

Answer 5

n Ne = grams/molar mass = ?

n Aar = grams/molar mass = ?

Then PV = mRT and use n Ne to solve for pNe. Use n for Ar to solve for pAr.