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Charra [1.4K]
3 years ago
9

250 g H 2 SO 4 completely reacted with aluminum?

Chemistry
1 answer:
Rasek [7]3 years ago
3 0

Answer: 290 g of aluminium sulphate is produced.

Explanation:

To calculate the moles :

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

\text{Moles of} H_2SO_4=\frac{250g}{98g/mol}=2.55moles

The balanced chemical reaction is:

2Al(s)+3H_2SO_4(aq)\rightarrow Al_2(SO_4)_3(aq)+3H_2(g)

According to stoichiometry :

3 moles of H_2SO_4 produce  = 1 mole of Al_2(SO_4)_3

Thus 2.55 moles of H_2SO_4 will require=\frac{1}{3}\times 2.55=0.85moles  of Al_2(SO_4)_3

Mass of Al_2(SO_4)_3=moles\times {\text {Molar mass}}=0.85moles\times 342g/mol=290g

Thus 290 g of aluminium sulphate is produced.

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Which of the following processes absorbs energy? A) condensation of water on a wind shield of a car B) formation of copperC) bal
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Answer:

C) ball rollinflown a hill

Explanation:

The question asks to  identify the endothermic process in the list of options. By way of elimination, we have;

A) condensation of water on a wind shield of a car

Condensation is an exothermic process. That is, heat is given out as the gases change into the liquid state of matter.

B) formation of copper

This is an exothermic process. Capture of electrons by a cation is always exothermic.

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This is the correct option. Energy is absorbed by the ball as it moves on the hill

D) formation of ice from liquid water

Freezing is an example of exothermic reaction. Heat is given off to the surroundings.

E) oxide from copper and oxygen

Formation of metal oxides and most reactions involving oxygen are exothermic reactions,

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3 years ago
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8 0
3 years ago
The most common source of copper (cu) is the mineral chalcopyrite (cufes2). how many kilograms of chalcopyrite must be mined to
tigry1 [53]

Answer : 0.8663 Kg of chalcopyrite must be mined to obtained 300 g of pure Cu.

Solution : Given,

Mass of Cu = 300 g

Molar mass of Cu = 63.546 g/mole

Molar mass of CuFeS_2 = 183.511 g/mole

  • First we have to calculate the moles of Cu.

\text{ Moles of Cu}=\frac{\text{ Given mass of Cu}}{\text{ Molar mass of Cu}}= \frac{300g}{63.546g/mole}=4.7209moles

The moles of Cu = 4.7209 moles

From the given chemical formula, CuFeS_2 we conclude that the each mole of compound contain one mole of Cu.

So, The moles of Cu = Moles of CuFeS_2 = 4.4209 moles

  • Now we have to calculate the mass of CuFeS_2.

Mass of CuFeS_2 = Moles of CuFeS_2 × Molar mass of CuFeS_2 = 4.4209 moles × 183.511 g/mole = 866.337 g

Mass of CuFeS_2 = 866.337 g = 0.8663 Kg         (1 Kg = 1000 g)

Therefore, 0.8663 Kg of chalcopyrite must be mined to obtained 300 g of pure Cu.


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3 years ago
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