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ipn [44]
3 years ago
10

A gas mixture contains 0.150 mol of O2 gas, 0.116 mol of N2 gas, and 0.211 mol of Ar gas in a 0.500 L flask at 298 K. What is th

e partial pressure of N2 the mixture?

Chemistry
1 answer:
miskamm [114]3 years ago
4 0

Answer:

The partial pressure of N₂ in the mixture is 5.67 atm

Explanation:

According to Dalton's law, the partial pressure of a gas in a mixture of gases is given by the formula;

Partial pressure of gas A = Mole fraction of gas A × Total pressure of the mixture

We are required to calculate the partial pressure of N₂ in the mixture;

We are going to use the following simple steps;

Step 1. Calculating the total pressure of the mixture

We are given;

Moles of O₂ = 0.150 mol

Moles of N₂ = 0.116 mol

Moles of Ar = 0.211 mol

Thus , total moles of the mixture =  0.150 mol +0.116 mol + 0.211 mol

                                                      = 0.477 mol

Volume of the flask = 0.5 L

Temperature = 298 K

But; PV = nRT , where n is the number of moles and R is the ideal gas constant,0.082057 L.atm/mol.K

Thus; P = nRT ÷ V

            = (0.477 mol × 0.082057 × 298 )÷ 0.5

            = 23.328 atm

Step 2: Mole fraction of N₂

Mole fraction of a gas = Moles of a gas ÷ Total moles of the mixture

Mole fraction of N₂ = 0.116 mol ÷ 0.477 mol

                               = 0.243

Step 3: Partial pressure of N₂

P(N₂) = Mole fraction of N₂ × P(total)

       = 0.243 × 23.328 atm

       = 5.669 atm

       = 5.67 atm ( 2 d.p.)

Therefore, the partial pressure of N₂ in the mixture is 5.67 atm

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A boy inflated a bunch of balloons while he was outside with an ambient temperature of 26oC. He then took the balloons inside hi
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3 years ago
Solve the ideal gas law equation for pressure.
posledela

Answer:

p=\frac{nRT}{V}

Explanation:

The ideal gas law equation is an equation that relates some of the quantities that describe a gas: pressure, volume and temperature.

The equation is:

pV=nRT

where

p is the pressure of the gas

V is the volume of the gas

n is the number of moles of the gas

R is the gas constant

T is the absolute temperature of the gas (must be expressed in Kelvin)

Here we want to solve the equation isolating p, the pressure of the gas.

We can do that simply by dividing both terms by the volume, V. We find:

p=\frac{nRT}{V}

So, we see that:

- The pressure is directly proportional to the temperature of the gas

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6 0
3 years ago
If the fugacity of a pure component at the conditions of an ideal solution is 40 bar and its mole fraction is 0.4, what is its f
yaroslaw [1]

Answer : The fugacity in the solution is, 16 bar.

Explanation : Given,

Fugacity of a pure component = 40 bar

Mole fraction of component  = 0.4

Lewis-Randall rule : It states that in an ideal solution, the fugacity of a component is directly proportional to the mole fraction of the component in the solution.

Now we have to calculate the fugacity in the solution.

Formula used :

f_i=X_i\times f_i^o

where,

f_i = fugacity in the solution

f_i^o = fugacity of a pure component

X_1 = mole fraction of component

Now put all the give values in the above formula, we get:

f_i=0.4\times 40\text{ bar}

f_i=16\text{ bar}

Therefore, the fugacity in the solution is, 16 bar.

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3 years ago
If two gases a and b in separate 1 liter containers
Anton [14]

The pressure exerted when both gases are put together in a single 1 liter container is 5 atm.

<h3>What is pressure?</h3>

Pressure is the force exerted by any object on another object.

Given that, a and b separate 1 liter containers and exert pressure of 2 atm and 3 atm respectively.

When both gases a and b exert together, the pressure then

2 atm + 3 atm = 5 atm.

Thus, the pressure exerted when both gases are put together in a single 1 liter container is 5 atm.

Learn more about pressure

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7 0
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