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2 years ago

If the partial pressure of the diatomic gas is 0.630 ATM what is the total pressure?

Chemistry

2 answers:

astraxan [27]2 years ago

8 0

3 moles of the diatomic green
--> p1=0.63 atm = 3×2 atoms
p2 is 6 moles of blue
p3 is 5 moles of orange
P-total (Pt) = p1 + p2 + p3
Pt = 0.63 + 0.63 + (0.63)(5)/6
Pt = 1.26 + 0.525 = 1.79 atm

11Alexandr11 [23.1K]2 years ago

8 0

Answer:

2.944 ATM

Explanation:

There are 14 molecules of gas mixture: 5 molecules of orange gas, 6 of blue gas and 3 of green gas. The green gas is the diatomic gas because it's formed by two atoms. The blue and the orange are monoatomic gases.

By the Dalton's Law, the partial pressure of a gas in a mixture of gas, may be calculeted knowing its molar fraction (Xi):

$Xi = \frac{molecules of the gas}{total molecules of the mixture} \\\\Xi = \frac{3}{14} \\\\Xi = 0.214$

Dalton's Law: Pi = Xi x Pt

0.630 = 0.214xPt

Pt = 2.944 ATM

Obs: The number of significant algorism such be the same of all parcels of the equation, including the result.

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2. If you have 8.08 g of hydrogen, how many grams of ammonia will your produce?

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answer: Stoichiometry is a big word for a process that chemist’s use to calculate

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 Stoichiometry calculates the quantities of reactants and products in a

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 Questions that deal with amounts in reactions are examples of reaction

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We just need to learn a new way to apply skills such as writing chemical

formulas, calculating formula masses, and converting from mass to moles,

particles to moles, and volume of gases to moles.

 Mole to Mole Conversions- you must have the Mole Ratio.

Illustration:

Let’s use an analogy that we can understand to begin to understand the process.

The KEY to any mole conversion is the ratio of coefficients in the reaction

equation. Say I want to make a bacon double cheeseburger. Let’s get our recipe

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2) How many bacon double cheeseburgers can you make if you start with:

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7 0

3 years ago

Calculate the second volumes 980L at 71C and 107.2atm to 13C and 59.3atm

Lapatulllka [165]

Answer:

V₂ = 1473.03 L

Explanation:

Given data:

Initial volume = 980 L

Initial pressure = 107.2 atm

Initial temperature = 71 °C (71 +273.15 = 344.15 K)

Final temperature = 13°C (13+273.15 = 286.15K)

Final volume = ?

Final pressure = 59.3 atm

Formula:

P₁V₁/T₁ = P₂V₂/T₂

Solution:

V₂ = P₁V₁ T₂/ T₁ P₂

V₂ = 107.2 atm × 980L × 286.15 K / 344.15 K× 59.3 atm

V₂ = 30061774.4 atm .L. K / 20408.095 atm. K

V₂ = 1473.03 L

5 0

3 years ago

A. 14.8

Scilla [17]

Answer:

Explanation:

Given data:

Initial volume = 2.5 L

Initial temperature = 300 k

Final temperature = 80 k

Final volume = ?

Solution:

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁

V₂ = 2.5 L × 80 K / 300 k

V₂ = 200 L.K / 300 K

V₂ = 0.67 L

Given data:

Initial volume = 752 mL

Initial temperature = 25.0°C (25+273 = 298 K)

Final temperature = 50.0°C(50+273 = 323 K)

Final volume = ?

Solution:

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁

V₂ = 752 mL × 323 K / 298 k

V₂ = 242896 mL.K / 298 K

V₂ = 815.1 mL

Given data:

Initial volume = 2.75 L

Initial temperature = 20°C (20+273 = 293 K)

Final temperature = ?

Final volume = 2.46 L

Solution:

The given problem will be solve through the Charles Law.

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

T₂ = V₂T₁/V₁

T₂ = 2.46 L × 293 K / 2.75 L

T₂ = 720.78 L.K / 2.75 L

T₂ = 262.1 K

Given data:

Initial volume = 1500 L

Initial temperature = 5°C (5+273 = 278 K)

Final temperature = 30 °C(30+273 = 303 K)

Final volume of heated air = ?

Solution:

The given problem will be solve through the Charles Law.

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁

V₂ = 1500 L × 303 K / 278 k

V₂ = 454500 L.K / 278 K

V₂ = 1634.89 L

Given data:

Initial volume = 15.5 L

Initial temperature = 20°C (20+273 = 293 K)

Final temperature = 7.0 °C(7.0+273 = 280 K)

Final volume of balloon = ?

Solution:

The given problem will be solve through the Charles Law.

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁

V₂ = 15.5 L × 280 K / 293 k

V₂ = 4340 L.K / 293 K

V₂ = 14.8 L

Given data:

Initial volume = 150 mL

Initial temperature = 23.5°C (23.5+273 = 296.5 K)

Final temperature = 72.5 °C(72.5+273 = 345.5 K)

Final volume of balloon = ?

Solution:

The given problem will be solve through the Charles Law.

V₁/T₁ = V₂/T₂

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T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₂ = V₁T₂/T₁

V₂ = 150 mL × 345.5 K / 296.5 k

V₂ = 51825 mL.K / 296.5 K

V₂ = 174.79 mL

6 0

3 years ago

We have a methanol solution that is 6.0 m methanol, CH 3OH in water. Vapor pressure pure water at 30. degrees C is 31.82 mmHg. V

Mashcka [7]

<u>Answer:</u> The total pressure above the solution at 30°C is 45.29 mmHg

<u>Explanation:</u>

We are given:

Molality of methanol = 6.0 m

This means that 6.0 moles of methanol present in 1 kg or 1000 g of pure water

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of water = 1000 g

Molar mass of water = 18 g/mol

Putting values in above equation, we get:

$\text{Moles of water}=\frac{1000g}{18g/mol}=55.56mol$

Mole fraction of a substance is given by:

$\chi_A=\frac{n_A}{n_A+n_B}$

$\chi_{CH_3OH}=\frac{n_{CH_3OH}}{n_{CH_3OH}+n_{water}}\\\\\chi_{CH_3OH}=\frac{6}{6+55.56}=0.0975$

$\chi_{water}=\frac{n_{water}}{n_{CH_3OH}+n_{water}}\\\\\chi_{water}=\frac{55.56}{6+55.56}=0.9025$

To calculate the total pressure, we use the equation given by Dalton and Raoults, which is:

$p_T=(p_A\times \chi_A)+(p_B\times \chi_B)$

where,

$p_T$ = total vapor pressure = ?

We are given:

Mole fraction of methanol = 0.0975

Mole fraction of water = 0.9025

Vapor pressure of methanol = 170.0 mmHg

Vapor pressure of water = 31.82 mmHg

Putting values in above equation, we get:

$p_T=(170\times 0.0975)+(31.82\times 0.9025)\\\\p_T=45.29mmHg$

Hence, the total pressure above the solution at 30°C is 45.29 mmHg

6 0

3 years ago