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3 years ago

What pressure is required to compress 196.0 liters of air at 1.83 atmosphere into a cylinder whose volume is 26.0 liters

Chemistry

1 answer:

drek231 [11]3 years ago

5 0

Answer:

P₂ = 13.79 atm

Explanation:

Given data:

Initial volume = 196.0 L

Initial pressure = 1.83 atm

Final volume = 26.0 L

Final pressure = ?

Solution:

The given problem will be solved through the Boyle's law,

"The volume of given amount of gas is inversely proportional to its pressure by keeping the temperature and number of moles constant"

Mathematical expression:

P₁V₁ = P₂V₂

P₁ = Initial pressure

V₁ = initial volume

P₂ = final pressure

V₂ = final volume

Now we will put the values in formula,

P₁V₁ = P₂V₂

1.83 atm × 196.0 L = P₂× 26.0 L

P₂ = 358.68 atm. L / 26.0 L

P₂ = 13.79 atm

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Calculate the volume in liters of a ×1.0310−6mM silver(II) oxide solution that contains 900.mg of silver(II) oxide AgO.

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Answer : The volume of solution will be, $7.047\times 10^6L$

Explanation : Given,

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3 years ago

What usually happens to the outer electrons of metallic atoms when they combine chemically with nonmetallic atoms?

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How many valence electrons are in a phosphorous ION? Would it have a full shell?<br> A. 5<br> B. 8

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4 years ago

Read 2 more answers

How many grams of phosphorus are required to produce 4.21x10^22 molecules of phosphorus trifluoride?

kolezko [41]

2.1618 grams of P4 is required to produce 4.21x10^22 molecules of phosphorus trifluoride.

Explanation:

The balanced chemical reaction for formation of PF3 from yellow phosphorus is given by:

P4 + 6F2 ⇒ 4PF3

1 mole of P4 reacts to give 4 moles of PF3

It is given that 4.21x10^22 molecules of PF3 are produced

so the number of moles can be calculated by the relation

number of molecules = number of moles × Avagadro number

number of moles = $\frac{number of molecules}{avagadro number}$

n = $\frac{4.21x10^22}{6.023. 10^23}$

n= 0.06989 moles of PF3 is formed.

Applying stoichiometry,

1 mole of P4 gives 4 moles PF3

x mole will produce 0.06989 moles of PF3

$\frac{4}{1}$ = $\frac{0.0698}{x}$

4x= 0.0698 × 1

x = $\frac{0.0698}{4}$

x= 0.01745 moles of P4 will be required.

The weight of the phosphorus can be obtained by number of moles × atomic mass of one mole of P4

= 0.01745 × 123.89

= 2.1618 grams of P4.

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3 years ago