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3 years ago

Where does oxidation occur in an electrochemical cell?

Chemistry

2 answers:

Studentka2010 [4]3 years ago

6 0

Answer: (3) at the anode in both an electrolytic cell and a voltaic cell

Explanation: Electrolytic cells are the cells which convert electrical energy into chemical energy. For this purpose, 2 rods or electrodes are kept in the chemical solution. One is cathode and the other one is anode.

Anode is the electrode at which oxidation takes place and the sign of the electrode is positive and Cathode is the electrode at which reduction takes place and the sign of the electrode is negative.

Voltaic cells are the opposite of the electrolytic cell and both of the processes are same but the signs of the electrode are opposite. Anode is negatively charged and cathode is positively charged in this cell.

Thus option (3 is correct) as oxidation occurs at anode in both an electrolytic cell an voltaic cell.

crimeas [40]3 years ago

4 0

(3); try using the phrase "AN OX ate the RED CAT"
(anode=oxidation, reduction=cathode)

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Explain with suitable chemical reaction, oxidation & reduction is a simultaneus &

bagirrra123 [75]

Answer:

here's the answer hope it helps

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3 years ago

Calculate the amount of heat required for the evaporation of 105.0 g of water at 100.0 c

son4ous [18]

To determine the amount of heat needed to evaporate a certain amount of water at its boiling point, we use the equation,

H = m(Hv)

where H is the heat, m is the mass (in grams), and Hv is the latent heat of vaporization. Substituting the known values,

H = (105 g)(540 cal/g)

H = 56700 cal

H = 56.7 kcal

Answer: 56.7 kcal

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4 years ago

Use the formula for pressure to determine the weight of a box that creates a pressure of 1,065 N/cm2 when resting on a 17.0-cm2

Sloan [31]

Force /Area = Pressure
Force = Pressure * Area
Force = 1065 * 17 = 18105 N

weight = 18105 N

I hope this helps!

8 0

3 years ago

Read 2 more answers

2. An exothermic reaction releases 86.5 kJ. How many kilocalories of<br> energy are released?

Alenkasestr [34]

Answer:

20.67 kcal of energy is released.

Explanation:

It is given that, an exothermic reaction releases 86.5 kJ. We need to convet kJ to calories.

Since,

1 kcal = 4.184 kJ

So,

1 kJ = 0.239 kcal

For 86.5 kJ,

86.5 kJ = (0.239 × 86.5) kcal

86.5 kJ = 20.67 kcal

So, 20.67 kcal of energy is released.

7 0

3 years ago

When aluminum, AlAl, metal is dipped in an aqueous solution of hydrochloric acid, HClHCl, hydrogen gas, H2H2, is produced with t

kifflom [539]

Answer:

Balanced equation: $2Al(s)+6HCl(aq.)\rightarrow 2AlCl_{3}(aq.)+3H_{2}(g)$

Explanation:

Al is an metallic species with a standard reduction potential of -1.66 V( $E_{Al^{3+}\mid Al}^{0}=-1.66V$ ).
$H_{2}$ is present at the intermediate position in electrochemical series with a standard reduction potential of 0 V ( $E_{H^{+}\mid H_{2}}^{0}=0V$ ).

So, when Al is dipped in aqueous solution of HCl, Al is readily oxidized to produce $Al^{3+}$ whereas $H^{+}$ is reduced to $H_{2}$ .
Hence, as a whole, aqueous $AlCl_{3}$ and gaseous $H_{2}$ is produced as products.

Balanced equation: $2Al(s)+6HCl(aq.)\rightarrow 2AlCl_{3}(aq.)+3H_{2}(g)$

5 0

4 years ago