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3 years ago

How many moles of aluminum oxide would form if 12.5 moles of aluminum burned

Chemistry

1 answer:

jarptica [38.1K]3 years ago

7 0

Balance it:

So you need 2 Al and 3 O2 to make 2 Al2O3 (aluminum oxide).

I'm going to assume you have all the O2 you need.

Since 2 mols of Al is needed to make 2 mols of the product, it's a 1:1 ratio. You get as much aluminum oxide for as much aluminum you burn.

So 12.5 mols if there is not a lack of the O2.

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Who was Charles Darwin and what theory is he best known for?

Alona [7]

Answer:

Charles Darwin, in full Charles Robert Darwin, (born February 12, 1809, Shrewsbury, Shropshire, England—died April 19, 1882, Downe, Kent), English naturalist whose scientific theory of evolution by natural selection became the foundation of modern evolutionary studies.

Charles Darwin's theory of evolution states that evolution happens by natural selection. Individuals in a species show variation in physical characteristics. ... As a consequence those individuals most suited to their environment survive and, given enough time, the species will gradually evolve.

Explanation:

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3 years ago

What is the conecntration of Fe3 and the concentration of No3- present in the solution that result when 30.0 ml of 1.75M Fe(No3)

zvonat [6]

Answer:

$[Fe^{+3}]=0.700 M$

$[NO_{3}^{-}]=2.10 M$

Explanation:

Here, a solution of Fe(NO₃)₃ is diluted, as the total volume of the solution has increased. The formula for dilution of the compound is mathematically expressed as:

$C_{1}. V_{1}= C_{2}.V_{2}$

Here, C and V are the concentration and volume respectively. The numbers at the subscript denote the initial and final values. The concentration of Fe(NO₃)₃ is 1.75 M. As ferric nitrate dissociates completely in water, the initial concentration of ferric is also 1.75 M.

Solving for [Fe],

$[Fe^{+3}]=\frac{C_{1}.V_{1}}{V_{2} }$

$[Fe^{+3}]=\frac{(1.75).(30.0)}{45.0+30.0 }$

$[Fe^{+3}]=0.700 M$

For [NO₃⁻],

There are three moles of nitrate is 1 mole of Fe(NO₃)₃. This means that the initial concentration of nitrate ions will be three times the concentration of ferric nitrate i.e., it will be 5.25 M.

$[NO_{3}^{-}]=\frac{C_{1}.V_{1}}{V_{2} }$

$[NO_{3}^{-}]=\frac{(5.25)(30.0)}{30.0+45.0 }$

$[NO_{3}^{-}]=2.10 M$

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3 years ago

If 110g of copper sulphate is present in 550g of solution calculate the concentration of solution

Bingel [31]

Answer:

20%

Explanation:

mass by mass percentage of a solution =(mass of solute)/(mass of solution)

mass of solute=550g

therefore 110×100/550=20%

hope u will understand .:") credit to the owner

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3 years ago

: Calculate molar mass of the following compounds:

lozanna [386]

Answer:

1. 58.5g/mol

2. 261g/mol

3. 158g/mol

4. 71g/mol

5. 44g/mol

Explanation:

The molar mass of a compound is the total mass of the sum of masses of all individual elements that make up the compound. First, we need to know the atomic masses of each element in a compound.

1. NaCl

Where; Na = 23, and Cl = 35.5

Molar mass of NaCl = 23 + 35.5

= 58.5g/mol

2. Ba(NO3)2:

Where; Ba = 137, N = 14, O = 16

Molar mass of Ba(NO3)2: 137 + {14 + 16(3)} 2

137 + (14 + 48)2

137 + (62)2

137 + 124

= 261g/mol

3. K(MnO4)

Where; K = 39, Mn = 55, O = 16

Molar mass of KMnO4 = 39 + 55 + 16(4)

= 94 + 64

= 158g/mol

4. Cl2

Where; Cl = 35.5

Molar mass of Cl2 = 35.5(2)

= 71g/mol

5. CO2

Where; C = 12, O = 16

Molar Mass of CO2 = 12 + 16(2)

= 12 + 32

= 44g/mol

3 0

3 years ago

All of the following are examples of a heterogeneous mixture EXCEPT:

CaHeK987 [17]

I think the answer is either a or d i haven't taken that class in awhile but if i were to pick one it would be D

3 0

3 years ago

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How many moles of aluminum oxide would form if 12.5 moles of aluminum burned​

How many moles of aluminum oxide would form if 12.5 moles of aluminum burned