Question

PLEASE HELP ASAP for 75 points

A 5.00 L flask is charged with 63.45 grams of I₂ and 2.5 atm of F₂ at 25°C. The flask is heated to 100°C until one of the reagents is completely consumed. What will be the total pressure (in atm) of the final products in the flask at 100°C?

Answer 1

Based on the calculations, the total pressure of the final products is equal to 1.76 atm.

How to calculate the total pressure (in atm)?

From the information provided about this chemical reaction, we can logically deduce the following parameters:

• Volume, V = 5.00 L.

• Mass, m of I₂ = 63.45 grams.

• Pressure, P  of F₂ = 2.5 atm.

• Initial temperature, t₁ = 25°C.

• Final temperature, t₂ = 100°C.

Next, we would write the properly balanced chemical equation for this chemical reaction:

                               I₂ + 5F₂   ⇒  2IF₅

Also, we would determine the number of moles of each atom of I₂ and F₂:

$Number \;of \;moles = \frac{mass}{molar\;mass}$

Substituting the given parameters into the formula, we have;

Number of moles = 63.45/253.8

Number of moles = 0.25 moles.

Assuming I₂ were limiting, we would need:

5 × 0.25 = 1.25 moles of F₂.

For fluorine gas, we have:

PV = mRT/MM

Mass, m = PVMM/RT

Mass, m = 2.5(5.00)(38)/(0.0821 × 298)

Mass, m = 475/24.4658

Mass, m = 19.42 grams.

Number of moles = 19.42/38

Number of moles = 0.51 moles.

The total number of moles = 0.25 + 0.51 = 0.76 mol.

For the mole fraction of I₂, we have:

Mf = 0.25/0.76

Mole fraction = 0.33.

For the mole fraction of F₂, we have:

Mole fraction = 1 - 0.33 = 0.67.

Next, we would determine the total pressure of the two elements by applying Dalton's law:

Total pressure = 0.33 × 0.27 + 0.67 × 2.5

Total pressure = 1.76 atm.

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