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2 years ago

Calculate the number of moles CuCl2 necessary to make 50 mL of a 0.15M solution

1 answer:

3 0

Volume ⇒ 50 mL in liters : 50 / 1000 = 0.05 L

Molarity of solution ⇒ 0.15 M

Number of moles:

n = M * V

n = 0.15 * 0.05

n = 0.0075 moles of CuCl2

hope this helps!.

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(03.02 MC) A student made the Lewis dot diagram of a compound as shown. Ca is written with two dots shown on its top. Cl is writ

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2 years ago

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Answer: Non-renewable energy comes from sources that will run out or will not be replenished in our lifetimes—or even in many, many lifetimes.

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2 years ago

A solution is prepared by dissolving 32. 0 g of NiSO4 in water. What current would be needed to deposit all of the nickel in 5.

strojnjashka [21]

The current needed to deposit all of the nickel in 5 hours is 2.219 A

<h3>What is Faraday's Law of electrolysis?</h3>

According to the first law of Faraday, the amount of substance liberated at an electrode is directly proportional to the quantity of charge passed through an electrolyte.

m = zq , where z = electrochemical equivalent

An electrochemical equivalent is the mass of the substance liberated at an electrode when 1 Columb of charge is passed through the electrolyte.

For the nickel,

$Ni^{2+} (aq) + 2e^- \rightarrow Ni (s)$

z = 2

The molar mass of NiS0₄ = 154.75 g

154.75 g of Ni needs 2 x 96485 C

32 g of Ni needs $\frac{2\times 96485\times 32}{154.75} \\$

32 g of Ni needs 39944.79 C

We know,

q = It

Where q = charge

I = current and t = time in seconds

q = 39944.79 C and t = 5 x 60 x 60 = 18000 s

$I = \frac{q}{t} \\ = \frac{39944.79}{18000}$

= 2.219 A

Hence, the current needed to deposit all the nickel is 2.219 A in 5 hours

Learn more about Faraday's law of electrolysis:

brainly.com/question/14548624

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1 year ago