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7 months ago

At STP what is the volume of 16.34 grams of nitrogen gas?

Chemistry

1 answer:

nika2105 [10]7 months ago

6 0

Answer:

Volume = 13.06 L

Explanation:

We are given: mass of nitrogren gas = 16.34 g

We know: molar mass of nitrogen gas = 28.014 g/mol

: ideal gas law constant = 0.082 L.atm/K.mol

At STP: temperature = 273.15 K

: pressure = 1 atm

We first determine the number of moles of nitrogen gas:

n = m/M

= 16.34/28.014

= 0.58 mol

Using the ideal gas law:

$\begin{gathered} PV\text{ = nRT} \\ \\ \therefore V\text{ = }\frac{nRT}{P}\text{ = }\frac{0.58\times0.082\times273.15}{1}\text{ = 13.06 L} \end{gathered}$

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Rama09 [41]

Answer:

Vapor pressure of solution → 151.1 Torr

Option 2.

Explanation:

Raoult's Law is relationed to colligative property about vapor pressure. A determined solute, can make, the vapor pressure of solution decreases.

ΔP = P° . Xm

where Xm is the mole fraction of solute, P° (vapor pressure of pure solvent)

and ΔP = Vapor pressure of pure solvent - Vapor pressure of solution.

In order to determine the vapor pressure of solution, we need to determine, the vapor pressure of B and A in the solution

B's pressure = P° B . Xm

When we add A to B, A works as the solute and B, as the solvent.

Vapor pressure of pure B is 135 torr. (P° B)

In order to determine, the Xm, we use the moles of A and B

Xm = 5.3 mol of B / (1.28 + 5.3) → 0.806

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If mole fraction of B is 0.806, mole fraction for A (solute) will be (1 - 0.806)

A's pressure = 218 Torr . 0.194 → 42.3 Torr

Vapor pressure of solution is sum of vapor pressures of solute + solvent.

Vapor pressure of solution = 42.3 Torr + 108.81 Torr → 151.1 Torr

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