What volume of a 0.550 M solution of potassium hydroxide (KOH) can be made with 19.9 g of potassium hydroxide?
1 answer:
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Answer:
The correct answer is B.
Explanation:
Heterogeneous equilibrium is that in which reagents and products are present in more than one phase.
When the reaction is carried out in a closed container, three equilibrium phases are present: solid magnesium oxide, solid magnesium sulfate and gaseous sulfur trioxide.
Hence, the equilibrium contant is given by:
The concentrations in the equilibrium equation are the relationships of the real concentrations between the concentrations in the standard state. Since the standard state of a pure solid is the pure solid itself, the ratio of concentrations for a pure solid is equal to one.
Now, we analyse each statement:
I) As the reaction is endothermic (ΔH>0), increasing the temperature shifts the balance to the right because excess heat will be used to form more products.
II) Increasing the volume will decrease the concentration of SO₃, so Q>K and then this shifts the balance to the left.
III) As it is a heterogeneous balance, adding MgO will not affect the balance.
IV) Removing SO3 will decrease its concentration and therefore the reaction equilibrium will shift to the left.
Answer:
You need 8,53 L of ammonia
Explanation:
Global reaction of remotion of nitrogen oxide with ammonia is:
4 NH₃ + 6 NO ⇒ 5 N₂ + 6 H₂O
This balanced equation shows that 4 NH₃ moles reacts with 6 NO moles.
With 100% yield and temperature and pressure constants it is possible to apply Avogadro's law. This law is an experimental gas law relating the volume of a gas to the amount of substance of gas present. The formula is:
Where:
V₁ is the NO volume = 12,8L
n₁ are NO moles = 6
n₂ are NH₃ moles = 4
V₂ is NH₃ volume, the unknown.
Thus, V₂ are 8,53 L of ammonia
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