Question

A container filled with a mixture fluorine gas and neon gas exerts a total pressure of 7.60 atm. There are 50.0 g of fluorine gas (F₂ ) in the container which exerts a pressure of 5.00 atm. To use Dalton's law of partial pressures, you have to compare molar quantities. What quantity in moles of fluorine gas are present in the container?

Answer 1

To find the moles of fluorine gas, divide its given mass (50.0 g) by its molar mass (38 g/mol) to obtain 1.32 mol. This value represents the quantity of fluorine gas in moles in the container according to Dalton's law of partial pressures.

Step-by-step explanation:

To calculate the quantity in moles of fluorine gas (F₂) present in the container, we can use the ideal gas law and Dalton's Law of Partial Pressures. Given 50.0 grams of F₂, we first need to find the molar mass of F₂. Fluorine has an atomic mass of approximately 19 u, so F₂ has a molar mass of 38 g/mol.

Next, we calculate the moles of F₂ using the formula:

moles of F₂ = mass (g) / molar mass (g/mol).

Therefore, we have:

moles of F₂ = 50.0 g / 38 g/mol = 1.32 mol of F₂.

This is the quantity in moles of fluorine gas present in the container. Using Dalton's law of partial pressures, we know that each gas in a mixture exerts a pressure independently, and the total pressure is the sum of the individual pressures. Here, the fluorine gas exerts a pressure of 5.00 atm.

Answer 2

To find the quantity in moles of fluorine gas in the container, we can use Dalton's law of partial pressures and set up a proportion using the given pressure values. By solving the proportion, we find that there are 76.0 moles of fluorine gas present.

Step-by-step explanation:

According to Dalton's law of partial pressures, the total pressure is equal to the sum of the partial pressures. In this case, the total pressure in the container is 7.60 atm and the pressure of the fluorine gas is 5.00 atm. To find the quantity in moles of fluorine gas, we can set up a proportion using the given pressure values:

(Moles of F₂) / (Total pressure) = (Moles of F₂ gas pressure) / (Fluorine gas pressure)

By plugging in the known values, we get:

(Moles of F₂) / (7.60 atm) = (50.0 g F₂) / (5.00 atm)

Now, we can solve for (Moles of F₂) by cross-multiplying:

(Moles of F₂) = (50.0 g F₂) * (7.60 atm) / (5.00 atm)

By calculating the expression, we find that there are 76.0 moles of fluorine gas present in the container.