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Readme [11.4K]
2 years ago
7

Which of the following is an oxidation-reduction reaction?

Chemistry
1 answer:
garik1379 [7]2 years ago
6 0

Answer:

D) Ba(s) + 2 HCl(aq) → BaCl2(aq) + H2(g)

Explanation:

In a redox reaction, One atom is gaining electrons (Reduction) whereas other is loosing electrons (Oxidation). In the reactions:

A) HBr(aq) + NaOH(aq) → NaBr(aq) + H2O(l)

As sodium is always +1 and Br always -1, <em>this is not a redox reaction.</em>

B) NaI(aq) + AgNO3(aq) → AgI(s) + NaNO3(aq)

Sodium is always +1 and nitrate ion is -1. <em>This is not a redox reaction</em>

C) Pb(C2H3O2)2(aq) + 2 LiBr(aq) → PbBr2(s) + 2 LiC2H3O2(aq)

Acetate ion, C2H3O2 is -1 as Br is -1, lithium is +1 and Pb +2, <em>This is not a redox reactoin</em>

<h3>D) Ba(s) + 2 HCl(aq) → BaCl2(aq) + H2(g)</h3>

Barium is 0 as Ba(s) but +1 as BaCl2. Is oxidizing

Hydrogen is +1 as HCl but 0 as H2. Is reducting.

This reaction is an oxidation-reduction reaction

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Liula [17]

None because Covalent compounds don’t conduct electricity because they are formed between the non metal atoms by sharing of electrons. The Covalent compounds haves no free electrons and also no ions and hence they do not conduct electricity. That is why they do not conduct electricity.

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3 years ago
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4vir4ik [10]

Answer: 25.8 g of Cl_2 will be produced from the decomposition of 73.4 g of AuCl_3

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}    

\text{Moles of} AuCl_3=\frac{73.4g}{303g/mol}=0.242moles

The balanced chemical reaction is:

2AuCl_3\rightarrow 2Au+3Cl_2  

According to stoichiometry :

2 moles of AuCl_3 produce =  3 moles of Cl_2

Thus 0.242 moles of  will produce= \frac{3}{2}\times 0.242=0.363mol of Cl_2

Mass of Cl_2= moles\times {\text {Molar mass}}=0.363mol\times 71g/mol=25.8g

Thus 25.8 g of Cl_2 will be produced from the decomposition of 73.4 g of AuCl_3

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2 years ago
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Explanation:

Charles's law is one of the gas laws which explains that at constant pressure, the temperature and volume of a gas are directly proportional to each other. According to kinetic theory, as temperature rises the kinetic energy of gas also increases proportionally

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Read 2 more answers
How many moles of H2O will be produced from 26.0 g of H2022<br> Stoichiome
lukranit [14]

Answer:

                       0.7644 moles of H₂O

Explanation:

                    The balance chemical equation is as follow;

                                      2 H₂O₂ → 2 H₂O + O₂

To solve this problem we will first calculate the moles of H₂O₂ as,

                           Moles  =  Mass / M/Mass

                           Moles  =  26.0 g / 34.01 g/mol

                           Moles  =  0.7644 mol

Secondly,

According to equation,

                      2 moles of H₂O₂ produces  =  2 moles of H₂O

Hence,

                0.7644 mol of H₂O₂ will produce  =  X moles of H₂O

Solving for X,

                        X  =  2 mol × 0.7644 mol / 2 mol

                       X =  0.7644 moles of H₂O

5 0
3 years ago
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