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makvit [3.9K]
2 years ago
15

A flask contains methane, chlorine and carbon monoxide gases. the partial pressures of each are 0.215 atm, 0.066 atm, and 0.826

atm, respectively. what is the total pressure in the flask in atm?
Chemistry
2 answers:
hjlf2 years ago
8 0

Answer;

The total pressure is 1.107 atm.

Explanation;

The total pressure is the sum of the pressures of the three gases in the flask

Pressure (total) = 0.215 atm + 0.066 atm + 0.826 atm = 1.107 atm

= 1.107 atm.

elixir [45]2 years ago
5 0

The law of partial pressures or Dalton's law, formulated the British chemist John Dalton in 1802, establishes that <u>the pressure of a mixture of gases</u>, that do not react chemically, <u>is equal to the sum of the partial pressures that each of them would exert if only one occupied the entire volume of the mixture</u>, without changing the temperature.

In this way, <u>Dalton's law can be used to determine the total pressure in a container that has a mixture of gases</u>, each of which exerts a partial pressure, considering that all gases behave like ideal gases.

According to Dalton's law, the total pressure in the flask will be,

P_{total} = P_{methane} + P_{chlorine} + P_{CO}

→ P_{total} = 0.215 atm + 0.066 atm + 0.826 atm

→ P_{total} = 1.107 atm

So, the total pressure in the flask is equal to 1.107 atm.

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Svetradugi [14.3K]
To determine the state of saturation of the solution, we calculate the mass of solute per mass of water for the given amounts and compare this value to the solubility. If the value is less than the solubility, then the solution is unsaturated. If it is greater than solubility, then it is supersaturated. If it is equal to the solubility, then it is saturated.

mass solute / mass water  = 39.0 grams K2SO4 / 225 grams H2O = 0.173 g K2SO4/ g H2O
solubility = 15 g /100 g = .15 g/g

Therefore, the solution is supersaturated. When it is shaken, some of the solute would precipitate out. 

mass of solute soluble to water = .15 g K2SO4/ g water ( 225 g water ) = 33.75 g K2SO4
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5 0
2 years ago
What mass of H2 gas (in <br> g. would be produced by the complete reaction of the aluminum block?
loris [4]

First lets calculate the moles of aluminum (molar mass is 27 gram/mol):

n = m/M = 14.9 / 27 = 0.551 mole of Al


According to the reaction between sulfuric acid and aluminum:

From 2 moles of aluminum ==> we get 3 moles of Hydrogen gas

so, let's do cross multiplication

0.551 ==> 0.551 * 3/2 = 0.83 mole of H2


So, from this reaction we got 0.83 mole of H2 gas

knowing that the molar mass of H2 is 2 gram/mol, the mass of the gas is.

m = n * M = 0.83 * 2 = 1.66 gram of H2


3 0
2 years ago
5. A Dumas bulb is filled with chlorine gas at the ambient pressure and is found to contain 7.1 g of chlorine when the temperatu
kati45 [8]

Answer:

a. The original temperature of the gas is 2743K.

b. 20atm.

Explanation:

a. As a result of the gas laws, you can know that the temperature is inversely proportional to moles of a gas when pressure and volume remains constant. The equation could be:

T₁n₁ = T₂n₂

<em>Where T is absolute temperature and n amount of gas at 1, initial state and 2, final states.</em>

<em />

<em>Replacing with values of the problem:</em>

T₁n₁ = T₂n₂

X*7.1g = (X+300)*6.4g

7.1X = 6.4X + 1920

0.7X = 1920

X = 2743K

<h3>The original temperature of the gas is 2743K</h3><h3 />

b. Using general gas law:

PV = nRT

<em>Where P is pressure (Our unknown)</em>

<em>V is volume = 2.24L</em>

<em>n are moles of gas (7.1g / 35.45g/mol = 0.20 moles)</em>

R is gas constant = 0.082atmL/molK

And T is absolute temperature (2743K)

P*2.24L = 0.20mol*0.082atmL/molK*2743K

<h3>P = 20atm</h3>

<em />

7 0
2 years ago
6. Un volumen de 1.0 mL de agua de mar contiene casi 4 x 10-12 g de Au. El volumen total de agua en los océanos es de 1.5 x 1021
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Answer:

The total amount of Au is $ 2.0\times10^{24}

Explanation:

Given that,

Mass of 1.0 ml of Au m=4\times10^{-2}\ g

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We need to calculate the volume in ml

Using given volume

V=1.5\times10^{21}\times1000\ mL

V=1.5\times10^{24}\ mL

We need to calculate the total mass of Au  

Using given data

1\ ml\ volume = 4\times10^{-2}\ g

1.5\times10^{24}\ ml=4\times10^{-2}\times1.5\times10^{24}

So, The total mass of Au is 6\times10^{22}\ g

The mass will be in ounce,

Mass=0.035274\times6\times10^{22}

Mass=2.12\times10^{21}\ ounce

The total amount of the Au Will be

Total\ amount=2.12\times10^{21}\times948

Total\ amount=2.0\times10^{24}

Hence, The total amount of Au is $ 2.0\times10^{24}

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The combustion of any hydrocarbon yields water and carbon dioxide. We will now construct a balanced equation:

C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

Each mole of propane requires 5 moles of oxygen.
4 0
2 years ago
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