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3 years ago

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Name of these two Alkanes

1 answer:

fgiga [73]3 years ago

5 0

3-ethyl-5,6-dimethyloctane

3-ethyl-2,3-dimethylpentane

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Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves

hjlf

This is an incomplete question, here is a complete question.

Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide:

$2MnCO_3(s)+O_2(g)\rightarrow 2MnO_2(s)+2CO_2(g)$

In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide:

$3MnO_2(s)+4Al(s)\rightarrow 3Mn(s)+2Al_2O_3(s)$

Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced.

Answer : The net chemical equation for the production of manganese is:

$6MnCO_3(s)+3O_2(g)+8Al(s)\rightarrow 6CO_2(g)+6Mn(s)+4Al_2O_3(s)$

Explanation :

The given two chemical reactions are:

(1) $2MnCO_3(s)+O_2(g)\rightarrow 2MnO_2(s)+2CO_2(g)$

(2) $3MnO_2(s)+4Al(s)\rightarrow 3Mn(s)+2Al_2O_3(s)$

First we are multiplying reaction 1 by 3, and reaction 2 by 2, we get:

(1)

(2) $6MnO_2(s)+8Al(s)\rightarrow 6Mn(s)+4Al_2O_3(s)$

Now we are adding both the reactions, we get the overall chemical reaction.

$6MnCO_3(s)+3O_2(g)+6MnO_2(s)+8Al(s)\rightarrow 6MnO_2(s)+6CO_2(g)+6Mn(s)+4Al_2O_3(s)$

The $MnO_2$ is common on both side, by cancelling it, we get:

The net chemical equation for the production of manganese is:

$6MnCO_3(s)+3O_2(g)+8Al(s)\rightarrow 6CO_2(g)+6Mn(s)+4Al_2O_3(s)$

5 0

4 years ago

What prevents most small meteoroids from hitting earth surface?

Ostrovityanka [42]

Gravity is the solution!. We are lucky to have Jupiter in our solar system. Jupiter's gravity is strong enough to pull meteorites towards itself.

4 0

3 years ago

An aqueous solution of barium hydroxide is standardized by titration with a 0.110 M solution of hydrochloric acid. If 29.5 mL of

Natali5045456 [20]

Answer:

0.02685 M is the molarity of the barium hydroxide solution.

Explanation:

To calculate the concentration of acid, we use the equation given by neutralization reaction:

$n_1M_1V_1=n_2M_2V_2$

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is $HCl$

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is $Ba(OH)_2$ mm.

We are given:

$n_1=11\\M_1=0.110 M\\V_1=14.4 mL\\n_2=2\\M_2=?\\V_2=29.5 mL$

Putting values in above equation, we get:

$1\times 0.11 M\times 14.4 mL=2\times M_2\times 29.5 mL$

$M_2=\frac{1\times 0.11 M\times 14.4 mL}{2\times 29.5 mL}=0.02685 M$

0.02685 M is the molarity of the barium hydroxide solution.

8 0

3 years ago

How many C atoms are there in a sample of C,H, that contains 6.59 x 1026 H atoms?

Flauer [41]

Answer:

bill gates

Explanation:

4 0

3 years ago

Can you help me with chemistry

Natali5045456 [20]

Maybe depends the question.

4 0

3 years ago