Limiting Reactant:
1 answer:
Zn as a limiting reactant
N₂ as an excess reactant
Theoretical Yield : 13.15 g
<h3>Further explanation</h3>Reaction
3 Zn + N₂ ⇒ Zn₃N₂
Ar Zn : 65,38 g/mol
Ar N₂ : 28.0134 g/mol
mol Zn
mol N₂
limiting reactant : the smaller ratio(mol:coefficient)
mol ratio Zn : N₂ :
Zn as a limiting reactant(smaller ratio)
N₂ as an excess reactant
mol Zn₃N₂ :
mass of Zn₃N₂ (Theoretical Yield) :
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Answer:
Explanation:
The Ideal Gas equation is:
(1)
Where:
is the pressure of the gas
the number of moles of gas
is the gas constant
is the absolute temperature of the gas in Kelvin.
is the volume
It is important to note that the behavior of a real gas is far from that of an ideal gas, taking into account that <u>an ideal gas is a single hypothetical gas</u>. However, under specific conditions of standard temperature and pressure (T=0\°C=273.15 K and P=1 atm=101,3 kPa) one mole of real gas (especially in noble gases such as Argon) will behave like an ideal gas and the constant R will be .
However, in this case we are not working with standard temperature and pressure, therefore, even if we are working with Argon, the value of R will be far from the constant of the ideal gases.
Having this clarified, let's isolate from (1):
(2)
Where:
is the absolute temperature of the gas in Kelvin.
(3)
Finally:
10.3 g of will produce from 12.7 g
.
In simple terms, a limiting reagent is a reactant that is completely used up in the reaction.
It is also referred to as a limiting reactant or limiting agent.
Now, according to the question,
Since it is a limiting reagent, it will react fully.
The mass of that will be produced will be:-
Equivalent mole of = Equivalent weight of
= 12.7/169.97 = x*2/274x = 10.3 g.
Hence, 10.3 g of will be produced.
It is used to restrict the reaction.
It tells you the estimated amount of compound to be used.
It brings quantitative understanding to chemical reactions.
More information on limiting reagents can be found here :
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