A chemist prepares a solution of silver perchlorate by measuring out of silver perchlorate into a volumetric flask and filling t
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0.498 moles of copper(II) phthalocyanine would be produced by
the complete cyclotetramerization of 255 grams of phthalonitrile in the
presence of excess copper(ll) chloride.
<em>Copper(ll) phthalocyanine (Cu(C₃₂H₁₆N₈)) is produced by the cyclotetramerization of phthalonitrile (C₈H₄N₂) according to the following reaction: 4 C₈H₄N₂(l) + CuCl₂(s) → Cu(C₃₂H₁₆N₈)(s) + Cl₂(g) How many moles of copper(II) phthalocyanine would be produced by the complete cyclotetramerization of 255 grams of phthalonitrile in the presence of excess copper(II) chloride?</em>
Let's consider the following balanced equation.
4 C₈H₄N₂(l) + CuCl₂(s) → Cu(C₃₂H₁₆N₈)(s) + Cl₂(g)
The molar mass of C₈H₄N₂ is 128.13 g/mol. The moles corresponding to 255 g of C₈H₄N₂ are:
The molar ratio of C₈H₄N₂ to Cu(C₃₂H₁₆N₈) is 4:1. The moles of Cu(C₃₂H₁₆N₈) produced from 1.99 moles of C₈H₄N₂ are:
0.498 moles of copper(II) phthalocyanine would be produced by
the complete cyclotetramerization of 255 grams of phthalonitrile in the
presence of excess copper(ll) chloride.
You can learn more about stoichiometry here: brainly.com/question/22288091
Answer:
is the value of the equilibrium constant at this temperature.
Explanation:
We are given:
Partial pressure of
Partial pressure of
Partial pressure of
The expression of for the given chemical equation is:
Putting values in above equation, we get:
is the value of the equilibrium constant at this temperature.