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3 years ago

How much time is needed to deposit 1.0 g of chromium metal from an aqueous solution of crcl3 using a current of 1.5 a?

2 answers:

8 0

The metal component of the given compound, CrCl3, is chromium. The number of moles per 1 g of chromium is calculated through the equation below,

n = (1 g Cr)(1 mol Cr/51.996 g Cr)
n = 0.0192 mol Cr(3 electrons/1 mol Cr)
n = 0.0577 e-

Determine the number in charge by multiplying with Faraday's constant,

C = (0.0577 mol Cr)((1 F/1 mol e-)(96485 C/ 1F)
C = 5,566.87 C

Then, calculate time by dividing the charge with the current,

t = 5566.87 C/1.5 A
t = 3711.25 minutes
t = 61.84 hours

<span><em>Answer: 61.84 hours</em></span>

sergiy2304 [10]3 years ago

3 0

Answer:

$t=406.2s=6.77min$

Explanation:

Hello,

At first, one must compute the CrCl3 moles by using its molecular mass:

$n_{CrCl_3}=1gCrCl_3*\frac{1molCrCl_3}{152.35gCrCl_3}=0.00632molCrCl_3$

Now, we can apply the following equation to compute the requested time, based on the Faraday's constant, the involved charge and the fed current:

$C=n_{CrCl_3}*F\\C=0.00632molCrCl_3*96485\frac{C}{molCrCl_3}\\C=609.3C\\C=I*t\\t=\frac{C}{I}=\frac{609.3C}{1.5C/s} \\t=406.2s=6.77min$

Best regards.

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3 years ago

An unknown compound with a molar mass of 223.94 g/mol consists of 32.18% c, 4.50% h, and 63.32% cl. find the molecular formula f

Dima020 [189]

The actual number of atoms of each element present in the molecule of the compound is represented by the formula known as molecular formula.

Molar mass of the unknown compound = 223.94 g/mol (given)

Mass of each element present in the unknown compound is determined as:

Mass of carbon, $C$ :

$\frac{32.18}{100}\times 223.94 = 72.06 g$

Mass of hydrogen, $H$ :

$\frac{4.5}{100}\times 223.94 = 10.08 g$

Mass of chlorine, $Cl$ :

$\frac{63.32}{100}\times 223.94 = 141.79 g$

Now, the number of each element in the unknown compound is determined by the formula:

$number of moles = \frac{given mass}{molar mass}$

Number of moles of $C$ :

$number of moles = \frac{72.06}{12} = 6.005 mole\simeq 6 mole$

Number of moles of $H$ :

$number of moles = \frac{10.08}{1} = 10.08 mole\simeq 10 mole$

Number of moles of $Cl$

$number of moles = \frac{141.79}{35.5} = 3.99 mole\simeq 4 mole$

Dividing each mole with the smallest number of mole, to determine the empirical formula:

$C_{\frac{6}{4}}H_{\frac{10}{4}}Cl_{\frac{10}{4}}$

$C_{1.5}H_{2.5}Cl_{1}$

Multiplying with 2 to convert the numbers in formula into a whole number:

So, the empirical formula is $C_{3}H_{5}Cl_{2}$ .

Empirical mass = $12\times 3+1\times 5+2\times 35.5 = 112 g/mol$

In order to determine the molecular formula:

n = $\frac{molar mass}{empirical mass}$

n = $\frac{223.94}{112} = 1.99 \simeq 2$

So, the molecular formula is:

$2\times C_{3}H_{5}Cl_{2} = C_{6}H_{10}Cl_{4}$

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3 years ago

How many electrons does it in lithium.

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3 years ago

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3 years ago

Do you know how much water could you get if you started with 250.0 grams of hydrogen?

Soloha48 [4]

The amount of water that could we get if you started with 250.0 grams of hydrogen is 2,250 grams.

<h3>What is moles - mass realation?</h3>

Moles (n) and mass of any substance are related to each other according to the given equation as:

n = W/M, where

W = given mass

M = molar mass

Given balanced chemical reaction is:

2H₂ + O₂ → 2H₂O

Moles of 250g of H₂ = 250g / 2g/mol = 125mol

From the stoichiometry of the reaction it is clear that,

2 moles of H₂ = produces 2 moles of H₂O

125 moles of H₂ = produces 125 moles of H₂O

Now mass of water will be calculated as:

Mass = (125mol)(18g/mol) = 2,250g

Hence required mass of water is 2,250 grams.

To know more about moles & mass, visit the below link:
brainly.com/question/24631381

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3 years ago