A mixture of 10.0g of Ne and 10.0g of Ar was kept in a 1.00 L container at 765 torr. Calculate partial pressure of Ar inside container
A) 508 torr
B) 257 torr
C) 614 torr
D) 125 torr
calculate the moles of each gas.
partial pressure Ne= molesNe/totalmoles * 765torr
partial pressure Ar= molesAr/totalmoles * 765 torr
total moles= moles of each added up. Just looking at the answers, and knowing there are many more moles of Ne than Ar (argon has twice atomic mass as Ne), my guess is 257torr, for Ar pressure. Work it out.
Why did the noble gases throw a party in a 1.00 L container? Because they wanted to have a "neon" and "argon" good time! Now let's find out the partial pressure of Ar in the container.
To calculate the partial pressure of Ar, we first need to find the mole fraction of Ar in the mixture. We can do this by dividing the moles of Ar by the total moles of both Ne and Ar.
The moles of Ne can be calculated using the molar mass of Ne:
moles of Ne = mass of Ne / molar mass of Ne
Similarly, the moles of Ar can be calculated using the molar mass of Ar:
moles of Ar = mass of Ar / molar mass of Ar
Now, let's calculate the moles of Ne and Ar:
moles of Ne = 10.0g / molar mass of Ne
moles of Ar = 10.0g / molar mass of Ar
Next, we need to calculate the total moles of Ne and Ar:
total moles = moles of Ne + moles of Ar
Now, we can calculate the mole fraction of Ar:
mole fraction of Ar = moles of Ar / total moles
Finally, let's find the partial pressure of Ar using the ideal gas law:
partial pressure of Ar = mole fraction of Ar * total pressure
Is it time for the grand reveal? Drumroll, please... The partial pressure of Ar inside the container is **Option B) 257 torr**. Ar, that's a good one!
To calculate the partial pressure of argon (Ar) inside the container, we need to consider the mole fraction of argon in the mixture and multiply it by the total pressure.
Step 1: Calculate the moles of neon (Ne) and argon (Ar) using their given masses and molar masses.
Molar mass of Ne = 20.18 g/mol
Molar mass of Ar = 39.95 g/mol
Moles of Ne = mass of Ne / molar mass of Ne
= 10.0 g / 20.18 g/mol
= 0.495 mol
Moles of Ar = mass of Ar / molar mass of Ar
= 10.0 g / 39.95 g/mol
= 0.250 mol
Step 2: Calculate the total moles of gas in the mixture.
Total moles = moles of Ne + moles of Ar
= 0.495 mol + 0.250 mol
= 0.745 mol
Step 3: Calculate the mole fraction of argon (Ar) in the mixture.
Mole fraction of Ar = moles of Ar / total moles
= 0.250 mol / 0.745 mol
= 0.3356
Step 4: Calculate the partial pressure of argon (Ar) using the mole fraction and total pressure.
Partial pressure of Ar = mole fraction of Ar * total pressure
= 0.3356 * 765 torr
≈ 257 torr
Therefore, the partial pressure of argon (Ar) inside the container is approximately 257 torr.
The correct answer is option B) 257 torr.
To calculate the partial pressure of Ar inside the container, we need to use the concept of mole fraction.
Mole fraction is defined as the ratio of moles of a particular gas to the total moles of all gases present in the mixture.
First, we need to find the moles of Ne and Ar in the mixture. We can use the formula:
moles = mass / molar mass
The molar mass of Ne is 20.18 g/mol, so the moles of Ne can be calculated as:
moles of Ne = 10.0 g / 20.18 g/mol = 0.495 moles
Similarly, the molar mass of Ar is 39.95 g/mol, so the moles of Ar can be calculated as:
moles of Ar = 10.0 g / 39.95 g/mol = 0.250 moles
Next, we need to calculate the total moles of gas in the mixture:
total moles of gas = moles of Ne + moles of Ar = 0.495 moles + 0.250 moles = 0.745 moles
Now, we can calculate the mole fraction of Ar:
mole fraction of Ar = moles of Ar / total moles of gas = 0.250 moles / 0.745 moles = 0.336
Finally, we can use the mole fraction to calculate the partial pressure of Ar:
partial pressure of Ar = mole fraction of Ar * total pressure
The total pressure is given as 765 torr.
partial pressure of Ar = 0.336 * 765 torr = 257 torr
Therefore, the correct option is B) 257 torr.