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ziro4ka [17]
2 years ago
13

Can you please answer the question shown below?​

Chemistry
2 answers:
valentinak56 [21]2 years ago
8 0

Answer:

what is ur question tell me I will solve it

Yuki888 [10]2 years ago
6 0

Answer:

Nothing is shown below!!!

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How much<br>much hydrogen gas evolved<br>when 1.5 current is passed through water for 1.5 hours?​
evablogger [386]

0.042 moles of Hydrogen evolved

<h3>Further explanation</h3>

Given

I = 1.5 A

t = 1.5 hr = 5400 s

Required

Number of Hydrogen evolved

Solution

Electrolysis of water ⇒ decomposition reaction of water into Oxygen and Hydrogen gas.

Cathode(reduction-negative pole) : 2H₂O(l)+2e⁻ ⇒ H₂(g)+2OH⁻(aq)

Anode(oxidation-positive pole) : 2H₂O(l)⇒O₂(g)+4H⁻(aq)+4e⁻

Total reaction : 2H₂O(l)⇒2H₂(g)+O₂(g)

So at the cathode H₂ gas is produced

Faraday : 1 mole of electrons (e⁻) contains a charge of 96,500 C

\tt mol~e^-=\dfrac{Q}{96500}

Q = i.t

Q = 1.5 x 5400

Q = 8100 C

mol e⁻ = 8100 : 96500 = 0.084

From equation at cathode , mol ratio e⁻ : H₂ = 2 : 1, so mol H₂ = 0.042

4 0
3 years ago
Which of the following "spheres" is NOT involved in the water cycle?
olya-2409 [2.1K]
B is the correct answer.
The exosphere is the outermost region of the atmosphere the gradually merges out into space. The water cycle does not occur within this region.
5 0
3 years ago
Read 2 more answers
What is the mass of the hydrogen atoms in 1 mole of water
Katen [24]

<u>Answer:</u>

2.0158 grams

<u>Explantion:</u>

We are to find the mass of the hydrogen atoms in 1 mole of water.

We know that the formula of water is: H_2O

We can see, from the above mentioned formula, that water has 2 hydrpgen atoms.

From the periodic table, we get to know that Hydrogen has an atomic mass of 1.00794 grams.

As there are 2 atoms of hydrogen in water so 2 \times 1.00794 = 2.0158 grams is the answer

3 0
3 years ago
Read 2 more answers
I need it please !!!
anyanavicka [17]

Answer:

im pretty sure its 2...

Explanation:

if its wrong im sorry

if its right brainliest pls?

6 0
2 years ago
A 0.245-L flask contains 0.467 mol co2 at 159 °c. Calculate the pressure using the ideal gas law.
lubasha [3.4K]

Answer:

Pressure, P = 67.57 atm

Explanation:

<u>Given the following data;</u>

  • Volume = 0.245 L
  • Number of moles = 0.467 moles
  • Temperature = 159°C
  • Ideal gas constant, R = 0.08206 L·atm/mol·K

<u>Conversion:</u>

We would convert the value of the temperature in Celsius to Kelvin.

T = 273 + °C

T = 273 + 159

T = 432 Kelvin

To find the pressure of the gas, we would use the ideal gas law;

PV = nRT

Where;

  • P is the pressure.
  • V is the volume.
  • n is the number of moles of substance.
  • R is the ideal gas constant.
  • T is the temperature.

Making P the subject of formula, we have;

P = \frac {nRT}{V}

Substituting into the formula, we have;

P = \frac {0.467*0.08206*432}{0.245}

P = \frac {16.5551}{0.245}

<em>Pressure, P = 67.57 atm</em>

4 0
2 years ago
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