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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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How many moles of chlorine gas would occupy a volume of 35.5 L at a pressure of 100.0 kPa and a temperature of 100.0 degrees Cel
o-na [289]

1.137448506 mol moles of chlorine gas would occupy a volume of 35.5 L at a pressure of 100.0 kPa and a temperature of 100.0 degrees Celsius.

<h3>What is an ideal gas equation?</h3>

The ideal gas equation, pV = nRT, is an equation used to calculate either the pressure, volume, temperature or number of moles of a gas. The terms are: p = pressure, in pascals (Pa). V = volume, in m^3.

We apply the formula of the ideal gases, we clear n (number of moles); we use the ideal gas constant R = 0.082 l atm / K mol:

PV= nRT

Given data:

P=100.0 kPa =0.986923 atm

T=100 degree celcius= 100 + 273 =373 K

V=35.5 L

Substituting the values in the equation.

n= \frac{\;0,98 \;atm \;X \;35,5 \;L }{\;0,082\;atm / \;K mol \;X \;373 K}

n= 1.137448506 mol

Hence, 1.137448506 mol moles of chlorine gas would occupy a volume of 35.5 L at a pressure of 100.0 kPa and a temperature of 100.0 degrees Celsius.

Learn more about ideal gas here:

brainly.com/question/16552394

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7 0
2 years ago
How much energy does an X-ray with an 8 nm (8 x 10-9m) wavelength have?
myrzilka [38]

Answer:

it would be option C

Explanation:

Speed of light = 3×10^8m/s

Planck's constant = 6.626×10^-34 Js

Wavelength = 8 x 10^-9 m

Energy = [(3×10^8) * (6.626×10^-34)] / 8 x 10^-9

Energy = [19.878×10^(8-34)] / 8 x 10^-9

Energy = 2.48475 × 10^(-26+9)

Energy = 2.48×10^-17 J

3 0
3 years ago
If the volume occupied by the air in a bicycle pump is 525 cm3, and the pressure changes from 73.2 kPa to 122.5 k.Pa as the pist
Musya8 [376]

Answer:

V_2=313.71\ cm^3

Explanation:

Given that,

Initial volume, V_1=525\ cm^3

The pressure changes from 73.2 kPa to 122.5 k.Pa.

We need to find the new volume occupied by the air. Let it is V₂. It can be calculated using Boyle's law such that,

P_1V_1=P_2V_2\\\\V_2=\dfrac{P_1V_1}{P_2}\\\\V_2=\dfrac{73.2\times 525}{122.5}\\\\V_2=313.71\ cm^3

So, the new volume is 313.71\ cm^3.

6 0
2 years ago
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