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Nady [450]
2 years ago
15

A 2.0 L container of nitrogen gas had a pressure of 3.2 atm. What volume would be necessary to decrease the pressure to 1.0 atm

Chemistry
1 answer:
beks73 [17]2 years ago
6 0

Answer:

6.4 L

Explanation:

When all other variables are held constant, you can use Boyle's Law to find the missing volume:

P₁V₁ = P₂V₂

In this equation, "P₁" and "V₁" represent the initial pressure and volume. "P₂" and "V₂" represent the final pressure and volume. You can find the theoretical volume by plugging the given values into the equation and simplifying.

P₁ = 3.2 atm                      P₂ = 1.0 atm

V₁ = 2.0 L                          V₂ = ? L

P₁V₁ = P₂V₂                                                    <----- Boyle's Law

(3.2 atm)(2.0 L) = (1.0 atm)V₂                        <----- Insert values

6.4 = (1.0 atm)V₂                                           <----- Simplify left side

6.4 = V₂                                                        <----- Divide both sides by 1.0

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The volume (in mL) of calcium hydroxide, Ca(OH)₂ needed for the reaction is 19.8 mL

<h3>Balanced equation </h3>

2HCl + Ca(OH)₂ —> CaCl₂ + 2H₂O

From the balanced equation above,

  • The mole ratio of the acid, HCl (nA) = 2
  • The mole ratio of the base, Ca(OH)₂ (nB) = 1

<h3>How to determine the volume of Ca(OH)₂ </h3>
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MaVa / MbVb = nA / nB

(1.63 × 36) / (1.48 × Vb) = 2

58.68 / (1.48 × Vb) = 2

Cross multiply

2 × 1.48 × Vb = 58.68

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Divide both side by 2.96

Vb = 58.68 / 2.96

Vb = 19.8 mL

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Answer:

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Explanation:

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V_2 = Final volume = 1000 mL

M_1 = Initial concentration = 0.5 M

M_2 = Final concentration

We have the relation

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The new concentration is 0.05\ \text{M HCl}.

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