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3 years ago

10

What happens at the cathode in an electrolytic cell?

1 answer:

Aliun [14]3 years ago

3 0

Answer:

D. Reduction

Explanation:

In the electrolytic cell, reduction occurs at the cathode

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If a substance changes color, what has most likely happened

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say for example, the color of our blood inside the body is blue, when you have a cut, th he blood color is red through oxygenation.

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3 years ago

Two solid blocks are HEATED to the temperatures show. The blocks are placed so they touch. Which diagram shows the DIRECTION HEA

Setler [38]

Answer:

Heat flows from the block at high temperature to the one with lower temperature

Explanation:

The direction of heat flow is from a body at higher temperature to one with a lower temperature.

Temperature gradient determines the way and manner in which heat is dissipated.
As a system tend to increase entropy, it ensures that heat moves from hotter body to a colder body.
Heat movement here is by conduction as the body touches.
When both bodies reaches the same temperature, thermal equilibrium is established.

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3 years ago

What did Zoya and her freind do in response

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In response of what like what’s the full clear question

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3 years ago

One of the reactions that occurs in a blast furnace, in which iron ore is converted to cast iron, is Fe2O3 + 3CO → 2Fe + 3CO2 Su

Tpy6a [65]

Answer : The percent purity of $Fe_2O_3$ in the original sample is 87.94 %

Explanation :

The given balanced chemical reaction is:

$Fe_2O3+3CO\rightarrow 2Fe+3CO_2$

First we have to calculate the mass of Fe.

$\text{Moles of }Fe=\frac{\text{Mass of }Fe}{\text{Molar mass of }Fe}$

Molar mass of Fe = 55.8 g/mole

$\text{Moles of }Fe=\frac{1.79\times 10^3kg}{55.8g/mole}=\frac{1.79\times 10^3\times 1000g}{55.8g/mole}=3.15\times 10^4mole$

Now we have to calculate the moles of $Fe_2O_3$

From the balanced chemical reaction we conclude that,

As, 2 moles of Fe produced from 1 mole of $Fe_2O_3$

So, $3.15\times 10^4mole$ of Fe produced from $\frac{3.15\times 10^4}{2}=15750$ mole of $Fe_2O_3$

Now we have to calculate the mass of $Fe_2O_3$

$\text{ Mass of }Fe_2O_3=\text{ Moles of }Fe_2O_3\times \text{ Molar mass of }Fe_2O_3$

Molar mass of $Fe_2O_3$ = 159.69 g/mole

$\text{ Mass of }Fe_2O_3=(15750moles)\times (159.69g/mole)=2.515\times 10^6g=2.515\times 10^3kg$

Now we have to calculate the percent purity of $Fe_2O_3$ in the original sample.

Mass of original sample = $2.86\times 10^3kg$

$\text{Percent purity}=\frac{\text{Mass of }Fe_2O_3}{\text{Mass of sample}}\times 100$

$\text{Percent purity}=\frac{2.515\times 10^3kg}{2.86\times 10^3kg}\times 100=87.94\%$

Therefore, the percent purity of $Fe_2O_3$ in the original sample is 87.94 %

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3 years ago

Physicist Richard Feyneman used to say, "Science is a way of trying not to

Leokris [45]

Answer:

nope

Explanation:

nopeee

6 0

3 years ago