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murzikaleks [220]
3 years ago
6

What is the type of compound of copper and oxide?

Chemistry
1 answer:
kykrilka [37]3 years ago
5 0
Copper<span>(II) </span>oxide<span> or cupric </span>oxide<span> is the inorganic </span>compound<span> with the formula CuO. A black solid, it is one of the two stable </span>oxides<span> of </span>copper, the other being Cu2<span>O or cuprous </span>oxide<span>. As a mineral, it is known as tenorite and paramelaconite.</span>
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What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon
Varvara68 [4.7K]

Answer: 31.8 g

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}    

\text{Moles of} Al_2O_3=\frac{60.0g}{102g/mol}=0.59moles

\text{Moles of} C=\frac{30.0g}{12g/mol}=2.5moles

Al_2O_3+3C\rightarrow 2Al+3CO  

According to stoichiometry :

1 mole of Al_2O_3 require 3 moles of C

Thus 0.59 moles of Al_2O_3 will require=\frac{3}{1}\times 0.59=1.77moles  of C

Thus Al_2O_3 is the limiting reagent as it limits the formation of product and C is the excess reagent as it is present in more amount than required.

As 1 mole of Al_2O_3 give = 2 moles of Al

Thus 0.59 moles of Al_2O_3 give =\frac{2}{1}\times 0.59=1.18moles  of Al

Mass of Al=moles\times {\text {Molar mass}}=1.18moles\times 27g/mol=31.8g

Thus 31.8 g of Al will be produced from the given masses of both reactants.

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3 years ago
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Explanation:
1
2
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Whatever this molar quantity is, it is clear from the stoichiometry of the reaction that 3/2 equiv of dihydrogen gas were required. How much dinitrogen gas was required?
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