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3 years ago

11

Consider the following system at equilibrium.

1 answer:

Gelneren [198K]3 years ago

8 0

Answer:

Na₂CO₃.

Explanation:

<em>Le Châtelier's principle</em> states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.

The compound that has a common ion effect is Na₂CO₃.

When it is added to the solution, it is dissolved to produce Na⁺ and CO₃²⁻ which increases the concentration of CO₃²⁻ that will increase the concentration of the products side, so the reaction will be shifted to the left side to suppress the increase in the concentration of CO₃²⁻.

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This is an exercise in<u> the General Combined Gas Law</u>.

To start solving this exercise, we obtain the following data:

<h3>Data:</h3>

V₁ = 4.00 l
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P₁=Initial pressure
V₁=Initial volume
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T₂=end temperature
V₁=Initial temperature

We clear for final pressure (P2)

$\large\displaystyle\text{$\begin{gathered}\sf P_{2}=\frac{P_{1}V_{1}T_{2}}{V_{2}T_{1}} \ \ \to \ \ \ Formula \end{gathered}$}$

We substitute our data into the formula:

$\large\displaystyle\text{$\begin{gathered}\sf P_{2}=\frac{(365 \ mmHg)(4.00 \not{l})(303 \not{K})}{(2.80 \not{l})(293\not{K})} \end{gathered}$}$

$\large\displaystyle\text{$\begin{gathered}\sf P_{2}=\frac{442380 \ mmHg}{ 820.4 } \end{gathered}$}$

$\boxed{\large\displaystyle\text{$\begin{gathered}\sf P_{2}=539.224 \ mmHg \end{gathered}$}}$

Answer: The new canister pressure is 539.224 mmHg.

<h2>{ Pisces04 }</h2>

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