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3 years ago

What mass of hydrogen is produced from 5.71 mol of aluminum?

Chemistry

1 answer:

nasty-shy [4]3 years ago

5 0

Answer:

3.03 g

Explanation:

The first thing to do here is figure out the chemical formula for aluminium hydroxide.

Aluminium is located in group

of the periodic table, and forms

cations,

. The hydroxide anion,

−

, carries a

−

charge, which means that a formula unit of aluminium hydroxide will look like this

[

]

[

−

]

→

(

)

Now, you can figure out the mass of hydrogen present in

mole of aluminium hydroxide by first determining how many moles if hydrogen you get in

mole of aluminium hydroxide.

Since

mole of aluminium hydroxide contains

moles of hydroxide anions, which in turn contain

mole of hydrogen each, you can say that you will have

1 mole Al

(

)

→

moles OH

−

→

moles H

The problem tells you that the molar mass of hydrogen is equal to

1.01 g mol

−

. This means that

mole of hydrogen has a mass of

1.01 g

You can thus say that one mole of aluminium hydroxide contains

moles H

⋅

1.01 g

mole H

3.03 g H

∣

I'll leave the answer rounded to three sig figs. Btw my sister calculated this oof

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The first chemists, philosophers like, Aristotle were from which country?

qwelly [4]

Answer:

greece

Explanation:

aristole was particularly from stagria, greece. but most early philosophers are from greece

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3 years ago

how much water should be added to 1 gallon of pure antifreeze to obtain a solution that is 60% antifreeze?

antoniya [11.8K]

1 gallon of antifreeze = 60% of mixture. Total mixture:
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3 years ago

In a gas grill, 29 lbs propane C3H8 are

dimulka [17.4K]

Answer : The mass of combustion products formed are 134 lbs.

Explanation :

The balanced chemical reaction will be:

$C_3H_8+5O_2\rightarrow 3CO_2+4H_2O$

Given :

Mass of $C_3H_8$ = 29 lbs = 13154.2 g

conversion used : 1 lbs = 453.592 g

Molar mass of $C_3H_8$ = 44 g/mole

First we have to calculate the moles of $C_3H_8$ .

$\text{ Moles of }C_3H_8=\frac{\text{ Mass of }C_3H_8}{\text{ Molar mass of }C_3H_8}=\frac{13154.2g}{44g/mole}=298.9moles$

Now we have to calculate the moles of $CO_2$ and $H_2O$ .

From the balanced chemical reaction we conclude that,

As, 1 mole of $C_3H_8$ react to give 3 moles of $CO_2$

So, 298.9 mole of $C_3H_8$ react to give $298.9\times 3=896.7$ moles of $CO_2$

and,

As, 1 mole of $C_3H_8$ react to give 4 moles of $H_2O$

So, 298.9 mole of $C_3H_8$ react to give $298.9\times 4=1195.6$ moles of $H_2O$

Now we have to calculate the mass of $CO_2$ and $H_2O$ .

Molar mass of $CO_2$ = 44 g/mole

Molar mass of $H_2O$ = 18 g/mole

$\text{Mass of }CO_2=\text{Moles of }CO_2\times \text{Molar mass }CO_2$

$\text{Mass of }CO_2=896.7mole\times 44g/mole=39454.8g=86.98lbs$

and,

$\text{Mass of }H_2O=\text{Moles of }H_2O\times \text{Molar mass }H_2O$

$\text{Mass of }H_2O=1195.6mole\times 18g/mole=21520.8g=47.44lbs$

The total mass of products = Mass of $CO_2$ + Mass of $H_2O$

The total mass of products = 86.98 + 47.44 = 134.42 ≈ 134 lbs

Therefore, the mass of combustion products formed are 134 lbs.

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3 years ago

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Answer:

https://quizlet.com/199110979/biochem-chpt-5-flash-cards/

Explanation:

https://quizlet.com/199110979/biochem-chpt-5-flash-cards/

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3 years ago

why is deuterium-tritium reaction the most promising nuclear fusion reaction for future energy production?

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Answer:

The deuterium-tritium (DT, Figure 2) reaction is the most useful for fusion energy because it most easily overcomes the Coulomb repulsion, and it has the highest energy release among laboratory-feasible reactions.

Explanation:

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3 years ago