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Elis [28]
3 years ago
11

A 2.0 mol sample of ammonia is introduced into a 1.00 L container. At a certain temperature, the ammonia partially dissociates a

ccording to the equation: NH_3(g) N_2(g) + H_2(g) At equilibrium 1.00 mol of ammonia remains. Calculate the value for K.
Chemistry
1 answer:
aleksley [76]3 years ago
8 0

Answer:

K = 1.69M

Explanation:

For the reaction:

2NH₃(g) ⇄ N₂(g) + 3H₂(g)

K is defined as:

k = [N₂] [H₂]³ / [NH₃]² <em>(1)</em>

Molarity in equilibrium for each specie is:

NH₃(g): 2.0mol - 2x = 1.0mol/1L = 1M → X = 0.5mol

N₂(g): X = 0.5mol/1L = 0.5M

H₂(g): 3X = 1.5mol/1L = 1.5M

Replacing:

k = [0.5] [1.5]³ / [1]²

<em>k = 1.69M</em>

<em></em>

I hope it helps!

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Determine the mass of CO2 gas produced when 8.24 g of NaHCO3 is added to a solution that contains 4.41 g of HCl.
hjlf

The mass of CO₂ gas = 4.312 g

<h3>Further explanation</h3>

Reaction

NaHCO₃ (s) + HCl (aq) → NaCl (aq) + H₂O (aq) + CO₂ (g)

Find limiting reactant

mol NaHCO₃

\tt \dfrac{8.24}{84,007 }=0.098

mol HCl

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Limiting reactant :  NaHCO₃ (smaller)

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mass CO₂ :

\tt 0.098\times 44=4.312~g

4 0
3 years ago
A solution is prepared by dissolving 106.3 g HCl(g) in enough water to make 175.0 L of solution. The ph of this solution is
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Answer:

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If 100 ml of a 0.5 M HCI Solution is diluted with water to 1000ml, what is the new concetration?
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