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Mashcka [7]
4 years ago
15

Please Help!!!!!!!

Chemistry
1 answer:
hichkok12 [17]4 years ago
8 0

3,1,3,1

Explanation:

 Reaction equation:

    HBr    +    Al(OH)₃   ⇒    H₂O    +     AlBr₃

To balance an equation we make sure that the same number of atoms appears on both sides of the expression.

  HBr    +    Al(OH)₃   ⇒    H₂O    +     AlBr₃

Let us a simple mathematical method to solve this problem

  aHBr    +    bAl(OH)₃   ⇒    cH₂O    +     dAlBr₃

  a, b , c and d are the coefficients that will make the equation balanced;

 Conserving H;  a + 3b = 2c

                      Br;  a  = 3d

                      Al;   b  = d

                       O;    3b  = c

    let us make a = 1

                         d = \frac{1}{3}

                         b = \frac{1}{3}

                          c = 1

multiply through by 3;

     a = 3, b = 1, c= 3 and d = 1

learn more:

Balanced equation brainly.com/question/9325293

#learnwithBrainly

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Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction i
Natasha2012 [34]

Answer: Oxidation reaction:  Al(s)\rightarrow Al^{3+}(aq)+3e^-

Reduction reaction:  Sn^{2+}(aq)+2e^-\rightarrow Sn(s)

Overall redox reaction : 2Al(s)+3Sn^{2+}(aq)\rightarrow 2Al^{3+}(aq)+3Sn(s)

Explanation:

Oxidation-reduction reaction or redox reaction is defined as the reaction in which oxidation and reduction reactions occur simultaneously.

Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.

Al(s)\rightarrow Al^{3+}(aq)+3e^-

Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.

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Overall redox reaction : 2Al(s)+3Sn^{2+}(aq)\rightarrow 2Al^{3+}(aq)+3Sn(s)

5 0
3 years ago
3.364 g of hydrated barium chloride of BaCL2.xH2O was dissolved in water and made up to a total volume of 250.0 mL. 10.00 mL of
atroni [7]

<u>Given:</u>

Mass of hydrated barium chloride = 3.364 g

Total volume of barium chloride V(total)= 250 ml

Volume taken for titration V = 10 ml

Volume of AgNO3 consumed = 46.92 ml

Concentration of AgNO3 = 0.0253 M

<u>To determine:</u>

The value of x i.e. the water of hydration in BaCl2

<u>Explanation:</u>

The net ionic equation is-

Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

Based on the reaction stoichiometry: Equal moles of Ag+ and Cl- combine to form AgCl

Moles of Ag+ consumed = moles of Cl- present

Moles of Ag+ = V(AgNO3) * M(AgNO3) = 0.04692 * 0.0253 = 0.00119moles

Moles of Cl- present = 0.00119 moles

Thus, 0.00119 moles of Cl- are present in 10 ml of the solution

Therefore, number of moles of Cl- in 250 ml would be-

= 0.00119 * 250 /10 = 0.02975 moles of cl-

Now:

2 moles of Cl- are present in 1 mole of BaCl2

Therefore, 0.02975 moles of Cl- correspond to- 0.02975 * 1/2 = 0.01488 moles of BaCl2

Molar mass of BaCl2 = 208.22 g/mol

Thus, mass of BaCl2 = 0.01488 moles * 208.22 g.mol-1 = 3.098 g

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# moles of water 'x' = .266/18 = 0.015 ≅ 1

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7 0
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<h3>What are CAM?</h3>

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brainly.com/question/4170802

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