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Sloan [31]
3 years ago
13

Complete and balance the equation for this reaction in acidic solution. zns+no3-

Chemistry
1 answer:
Viefleur [7K]3 years ago
8 0
The equation given in question is as follow,

                                  ZnS + NO₃⁻    →    Zn²⁺ + S + NO

Oxidation state of elements in reactant side are as follow,
                                      Zn  =  +2
                                      S    =  -2
                                      N    =  +5
                                      O   =  -2
Oxidation state of elements in product side are as follow,
                                      Zn  =  +2
                                      S    =  0
                                      N    =  +2
                                      O   =  -2
So, In this reaction Nitrogen is Reduced while Sulfur is Oxidized.

Now Split the reaction into two half cell reactions,

Reduction Reaction,
                                ZnS     →     S  +  2e⁻
Oxidation Reaction,
                               NO₃⁻  +  3e⁻   →     NO

As the oxygen atoms are not balance, So, in acidic medium add H⁺ on the side having greater number of Oxygen atom and H₂O on the side having less number of Oxygen atoms,
Hence,
                                 H⁺  +   NO₃⁻  + 3e⁻    →     NO  +  H₂O
Now Balance the reaction,

                                 4H⁺  +   NO₃⁻  + 3e⁻    →     NO  +  2H₂O

So, write both half cell equations as,
 
                                             ZnS     →     S  +  2e⁻   --------- (1)
                               4H⁺  +   NO₃⁻  + 3e⁻    →     NO  +  2H₂O  -------(2)

Multiply eq. 1 with 3 and eq. 2 with 2 to equalize the electron.
So,
                                         3ZnS     →     3S  +  6e⁻   

                       8H⁺  +   2NO₃⁻  + 6e⁻    →     2NO  +  4H₂O 
                     _____________________________________(e⁻ cancelled)

                            3ZnS + 2NO₃⁻ + 8H⁺   → 3Zn + 3S + 2NO + 4H₂O
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When 45 g of an alloy, at 25oC, are dropped into 100.0 g of water, the alloy absorbs 956 J of heat. If the final temperature of
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Answer:

The answer to the question is

The specific heat capacity of the alloy = 1.77 J/(g·°C)

Explanation:

To solve this, we list out the given variables thus

Mass of alloy = 45 g

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Heat absorbed by the alloy = 956 J

Thus we have

ΔH = m·c·(T₂ - T₁) where  ΔH = heat absorbed by the alloy = 956 J, c = specific heat capacity of the alloy and T₁ = Initial temperature of the alloy = 25 °C , T₂ = Final temperature of the alloy = 37 °C  and m = mass of the alloy = 45 g

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3 years ago
If 2.68 g of benzaldehyde are involved with the mixed aldol condensation reaction, how many moles of benzaldehyde are present? R
Zielflug [23.3K]

Answer:

The number of moles of benzaldehyde = 0.0253 moles

Explanation:

The molecular formula of benzaldehyde is C₇H₆O

Its molecular mass is calculated from the atomic masses of the constituent atoms.

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Molecular mass = ( 12 * 7) + (1 * 6) + (16 * 1) = 106.0 g/mol

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Therefore, the number of moles of benzaldehyde = 0.0253 moles

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