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Viktor [21]
4 years ago
9

Consider the following general voltaic cell and a cell notation, and answer all three parts of this question.

Chemistry
1 answer:
Lubov Fominskaja [6]4 years ago
6 0

Answer:

<u>Part -1</u>

Electrode A - Mg(s)

Electrode B - Cl_{2}

<u>Part-2</u>

Option -C

<u>Part - 3</u>

Electrons flow from electrode -A to electrode -B.

Explanation:

<u>Part-1</u>

Electrode A is Mg(s)|Mg^{+2}(aq)

Electrode B is Cl_{2}(g)|Cl^{-}(aq)|C(s)

<u>Part-2</u>

From the electrode, magnesium looses two electrons and chlorine gains two electrons. Therefore, balanced redox equation for the voltaic cell is as follows.

Mg(s)+Cl_{2}(g)\rightarrow Mg^{2+}(aq)+2Cl^{-}(aq)

<u>Part-3</u>

<u>Na^{+} </u>ions flow from the left to right.

NO_{3}^{-} ions flow from the right to left.

Therefore, Electrons flow from electrode -A to electrode -B.

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Define self reduction reaction.
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4 years ago
1.What one factor identifies an atom as a specific element? . . Choices: the number of protons. . the atomic mass. . the number
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3 years ago
Stars with a greater overall mass are and , and they consume their nuclear fuel .
kozerog [31]

Answer:

they will expand

Explanation:

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3 years ago
A solution has a pOH of 12. Which best describes the solution?
Ray Of Light [21]

Answer:

The solution is acidic.

Explanation:

7 0
3 years ago
If 14.5 g of MnO4- (permanganate) react with manganese (II) hydroxide how many grams of manganese (IV) oxide will be produced? T
Veronika [31]

Answer:

m_{MnO_2}=21.2gMnO_2

Explanation:

Hello,

In this case, given the balanced reaction:

2MnO_4^-+2Mn(OH)_2\rightarrow 4MnO_2+2OH^-+H_2O

We can see a 2:4 mole ration between permanganate ion (118.9 g/mol) and manganese (IV) oxide (86.9 g/mol), that is why the resulting mas of this last one turns out:

m_{MnO_2}=14.5gMnO_4^-*\frac{1molMnO_4^-}{118.9gMnO_4^-}*\frac{4MnO_2}{2molMnO_4^-}  *\frac{86.9gMnO_2}{1molMnO_2} \\\\m_{MnO_2}=21.2gMnO_2

Best regards.

5 0
4 years ago
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