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borishaifa [10]
3 years ago
6

A balloon’s internal pressure is 1.25 atm, and its volume is 2.50 L. If the balloon is taken to the bottom of the ocean (pressur

e = 95.0 atm), what would be its new volume? Assume that the temperature does not change. (Round to the nearest hundredth place) L
Chemistry
2 answers:
Norma-Jean [14]3 years ago
6 0

Answer:

0.03 L 

Step-by-step explanation:

Since all other properties constant, we can use Boyle’s Law.

p₁V₁ = p₂V₂    Divide each side by p₂

   V₂ = V₁ × p₁/p₂

Data:

p₁ =     1.25 atm; V₁ = 2.50 L

p₂ = 95.0   atm; V₂ = ?

Calculations:

V₂= 1.25 × (2.50/95.0)

V₂= 1.25 × 0.026 32

V₂ ≈ 0.03 L

cricket20 [7]3 years ago
4 0

Where temperature is constant P1V1 = P2V2   where P = pressure and  V = volume.

so 1.25 * 2.5 = 95 * V2

V2 = (1.25 * 2.5) / 95

= 0.03  L to the nearest hundredth..

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Taking into account the scientific notation, the result of the sum is 10.84300×10³.

  • <u><em>Scientific notation</em></u>

First, remember that scientific notation is a quick way to represent a number using powers of base ten.

The numbers are written as a product:

a×10ⁿ

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15.24. Calcium hydroxide, also known as slaked lime, is used in industrial processes in which low concentrations of base are req
Ivahew [28]

The concentration of the hydroxide ions, OH¯ in 250 mL of the solution containing the maximum amount of dissolved calcium hydroxide is 0.01728 M

We'll begin by calculating the number of mole of in 0.16 g of Ca(OH)₂. This can be obtained as follow:

Mass of Ca(OH)₂ = 0.16 g

Molar mass of Ca(OH)₂ = 40 + 2[16 + 1] = 74 g/mol

<h3>Mole of Ca(OH)₂ =? </h3>

Mole = mass / molar mass

Mole of Ca(OH)₂ = 0.16 / 74

<h3>Mole of Ca(OH)₂ = 0.00216 mole </h3>

  • Next, we shall determine the molarity of the stock solution of Ca(OH)₂.

Mole of Ca(OH)₂ = 0.00216 mole

Volume = 100 mL = 100 / 1000 = 0.1 L

<h3>Molarity of Ca(OH)₂ =? </h3>

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Molarity of Ca(OH)₂ = 0.00216 / 0.1

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Volume of stock solution (V₁) = 100 mL

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<h3>Molarity of diluted solution (M₂) =?</h3>

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0.0216 × 100 = M₂ × 250

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Divide both side by 250

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Thus, the molarity of the diluted solution is 0.00864 M

  • Finally, we shall determine the concentration of the hydroxide ions, OH¯ in the diluted solution. This can be obtained as follow:

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From the balanced equation above,

1 mole of Ca(OH)₂ contains 2 moles of OH¯

Therefore,

0.00864 M Ca(OH)₂ will contain =  2 × 0.00864 = 0.01728 M OH¯

Thus, the concentration of the hydroxide ions, OH¯ in 250 mL of the solution containing the maximum amount of dissolved calcium hydroxide is 0.01728 M

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