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Gala2k [10]
3 years ago
15

Can you balance the following oxidation-reduction reaction and indicate which atoms have undergone oxidation and reduction? ____

HNO3 + ____S --> ____NO + ____H2SO4
Chemistry
2 answers:
Degger [83]3 years ago
8 0
Your coefficients are 2 1 2 1.
Illusion [34]3 years ago
4 0

Answer : The balanced oxidation-reduction reaction is,

2HNO_3+S\rightarrow 2NO+H_2SO_4

In this reaction, the 'S' atom shows oxidation and 'N' atom of HNO_3 shows reduction.

Explanation:

Redox reaction : It is a type of reaction in which an oxidation and reduction reaction takes palace simultaneously.

Oxidation : The loss of electrons and gain of oxygen or increase in the oxidation number is an oxidation.

Reduction : The gain of electrons and loss of oxygen or decrease in the oxidation number is a reduction.

The balanced redox reaction will be,

2HNO_3+S\rightarrow 2NO+H_2SO_4

From this we conclude that, the 'S' atom is oxidized due to increase in the oxidation number from 0 to (+6) and 'N' atom of HNO_3 is reduced due to decrease in the oxidation number from (+5) to (+2).  So, 'S' atom shows oxidation and 'N' atom shows reduction.

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Answer:

B

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Stationary front is a combination

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3 years ago
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3 years ago
What is the pH of 0.30 M ethanolamine, HOCH2CH2NH2, (Kb = 3.2 x 10−5)?
Dmitry [639]

Answer:

pH= 11.49

Explanation:

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From the question, the parameters given are; the concentration of ethanolamine which is = 0.30M, pH value= ??, pOH value= ??, kb=3.2 ×10^-5

Using the formula below;

[OH^-]=√(kb×molarity)----------------------------------------------------------------------------------------------------------(1)

[OH^-] =√(3.2×10^-5 × 0.30M)

[OH^-]= √(9.6×10^-6)

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8 0
3 years ago
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igomit [66]

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Explanation:

Hope this helps. :)

3 0
3 years ago
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