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hram777 [196]
3 years ago
12

What is the net redox reaction that occurs when Au comes into contact with acidic KMnO4? (Use the lowest possible coefficients.

Omit states-of-matter from your answer.)
Chemistry
1 answer:
Natalka [10]3 years ago
8 0

Answer:

3MnO₄⁻ + 24H⁺ + 5Au → 5Au³⁺ + 3Mn²⁺ + 12H₂O.

Explanation:

  • KMnO₄ is strong oxidizing agent which is reduced and oxidizes Au according to the two-half reactions:

The oxidation reaction: Au → Au³⁺ + 3e.

The reduction reaction: MnO₄⁻ + 8H⁺ + 5e → Mn²⁺ + 4H₂O.

  • To obtain the net redox reaction, we multiply the oxidation reaction by 5 and the reduction reaction by 5 to equalize the no. of electrons in the two-half reactions.

<em>So, the net redox reaction will be:</em>

<em>3MnO₄⁻ + 24H⁺ + 5Au → 5Au³⁺ + 3Mn²⁺ + 12H₂O.</em>

<em></em>

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Gaseous methane (CH4) reacts with gaseous oxygen gas (02) to produce gaseous carbon dioxide (CO2) and gaseous water (H20). What
Mariana [72]

Answer:

Theoretical yield = 3.51 g

Explanation:

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

For CH_4  :-

Mass of CH_4  = 1.28 g

Molar mass of CH_4  = 16.04 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{1.28\ g}{16.04\ g/mol}

Moles_{CH_4}= 0.0798\ mol

For O_2  :-

Mass of O_2  = 10.1 g

Molar mass of O_2  = 31.998 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{10.1\ g}{31.998\ g/mol}

Moles_{O_2}= 0.3156\ mol

According to the given reaction:

CH_4+2O_2\rightarrow CO_2+2H_2O

1 mole of methane gas reacts with 2 moles of oxygen gas

0.0798 mole of methane gas reacts with 2*0.0798 moles of oxygen gas

Moles of oxygen gas = 0.1596 moles

Available moles of oxygen gas = 0.3156 moles

<u>Limiting reagent is the one which is present in small amount. Thus, CH_4 is limiting reagent. </u>

The formation of the product is governed by the limiting reagent. So,

1 mole of methane gas on reaction produces 1 mole of carbon dioxide.

0.0798 mole of methane gas on reaction produces 0.0798 mole of carbon dioxide.

Mole of carbon dioxide = 0.0798 mole

Molar mass of carbon dioxide = 44.01 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

0.0798\ moles= \frac{Mass}{44.01\ g/mol}

Mass of CO_2 = 3.51 g

<u> Theoretical yield = 3.51 g</u>

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