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Helga [31]
3 years ago
7

Given the equation representing a chemical reaction at equilibrium in a sealed, rigid container:when the concentration of h2(g)

is increased by adding more hydrogen gas to the container at constant temperature, the equilibrium shifts
Chemistry
1 answer:
MrRa [10]3 years ago
5 0

Answer:

The equilibrium shifts to the right, shifting towards the products, thereby favouring forward reaction, leading to the production of more product (NH₃) and a reduction in the rate of backward reaction, resulting in a decrease in the production of reactant N₂ in the reaction.

Explanation:

Complete Question

Given the equation representing a chemical reaction at equilibrium in a sealed, rigid container:

N₂ (g) + H₂ (g) ⇌ NH₃ (g)

When the concentration of H₂(g) is increased by adding more hydrogen gas to the container at constant temperature, the equilibrium shifts

Solution

Le Chatelier's Principle explains the behaviour of the equilibrium in response to disturbances in properties for chemical reactions.

The principle states that, if the concentration, temperature and/or pressure of a chemical reaction at equilibrium is changed, the equilibrium position shifts to remedy this changes.

So, for a chemical reaction at equilibrium, provided that the other factors such as temperature and pressure remain constant, if more reactants are added (more H₂ is pumped into the reacting container), the equilibrium responds by shifting to the right, shifting towards the products, thereby favouring forward reaction, leading to the production of more product (NH₃) and a reduction in the rate of backward reaction, resulting in a decrease in the production of reactant N₂ in the reaction.

Hope this Helps!!!

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<u>Explanation:</u>

pH is the negative logarithm of hydronium ion concentration present in a solution.

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  • If the solution has low hydrogen ion concentration, then the pH will be high and the solution will be basic. The pH range of basic solution is 7.1 to 14
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To calculate the pH of the solution, we use equation:

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We are given:

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Now, putting values in equation 2, we get:

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  • <u>For 2:</u>

We are given:

pOH = 9.7

Putting values in equation 2, we get:

14 = 9.7 + pH

pH = 4.3

Now, putting values in equation 1, we get:

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The solution is acidic in nature.

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We are given:

pH = 7.0

Putting values in equation 1, we get:

7.0=-\log[H_3O^+]

[H_3O^+]=1.00\times 10^{-7}M

Now, putting values in equation 2, we get:

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pOH = 7.0

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  • <u>For 4:</u>

We are given:

pH = 12.9

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We are given:

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The solution is acidic in nature.

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