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omeli [17]
3 years ago
15

Write the balanced half equation of iron 2 and permanganate in a solution of acid. Show all of your work.

Chemistry
1 answer:
Aleks [24]3 years ago
6 0

Answer:

5Fe⁺² + MnO₄⁻ + 8H⁺ => 5Fe⁺³ + Mn⁺² + 4H₂O

Explanation:

Fe⁺² + MnO₄⁻ +  H⁺ => Mn⁺² + Fe⁺³ +  H₂O

5(Fe⁺² => Fe⁺³ + 1e⁻)      =>                        5Fe⁺² => 5Fe⁺³ + 5e⁻

<u>MnO₄⁻ + 5e⁻ => Mn⁺²    =>   MnO₄⁻ + 8H⁺ + 5e⁻ => Mn⁺² + 4H₂O</u>

                                      =>  5Fe⁺² + MnO₄⁻ + 8H⁺ => 5Fe⁺³ + Mn⁺² + 4H₂O

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A) Temperature does not affect reaction rate
6 0
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Which of the following chemical reactions will produce a precipitate?
Ilya [14]

Answer:

C

Explanation:

5 0
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When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced equation fo
Mashcka [7]

Answer:

The answer to your question is letter C.

Explanation:

Reaction

Potassium hydroxide = KOH

Barium chloride = BaCl₂

Potassium chloride = KCl

Barium hydroxide = Ba(OH)₂

           KOH   +   BaCl₂    ⇒    KCl   +   Ba(OH)₂

         Reactant        Elements       Products

               1                     K                      1

               1                     Ba                    1

               2                    Cl                     1  

                1                     H                    2

                1                     O                    2

The reaction is unbalanced

        2KOH   +   BaCl₂    ⇒   2KCl   +   Ba(OH)₂

         Reactant        Elements       Products

               2                     K                     2

               1                     Ba                    1

               2                    Cl                     2  

               2                      H                    2

               2                     O                    2

Now, the reaction is balanced

7 0
3 years ago
Read 2 more answers
The decomposition of HBr(g) into elemental species is found to have a rate constant of 4.2 ×10−3atm s−1. If 2.00 atm of HBr are
Dennis_Churaev [7]

Answer:

7,94 minutes

Explanation:

If the descomposition of HBr(gr) into elemental species have a rate constant, then this reaction belongs to a zero-order reaction kinetics, where the r<em>eaction rate does not depend on the concentration of the reactants. </em>

For the zero-order reactions, concentration-time equation can be written as follows:

                                          [A] = - Kt + [Ao]

where:

  • [A]: concentration of the reactant A at the <em>t </em>time,
  • [A]o: initial concentration of the reactant A,
  • K: rate constant,
  • t: elapsed time of the reaction

<u>To solve the problem, we just replace our data in the concentration-time equation, and we clear the value of t.</u>

Data:

K = 4.2 ×10−3atm/s,  

[A]o=[HBr]o= 2 atm,  

[A]=[HBr]=0 atm (all HBr(g) is gone)

<em>We clear the incognita :</em>

[A] = - Kt + [Ao]............. Kt =  [Ao] - [A]

                                        t  = ([Ao] - [A])/K

<em>We replace the numerical values:</em>

t = (2 atm - 0 atm)/4.2 ×10−3atm/s = 476,19 s = 7,94 minutes

So, we need 7,94 minutes to achieve complete conversion into elements ([HBr]=0).

6 0
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3 0
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