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Purification of nickel can be achieved by electrorefining nickel from an impure nickel anode onto a pure nickel cathode in an el

Alexxandr [17]

Answer: 530 hours

Explanation:

The reduction of Nickel ions to nickel is shown as:

$Ni^{2+}+2e^-\rightarrow Ni$

$96500\times 2=193000Coloumb$ of electricity deposits 1 mole of Nickel

1 mole of Nickel weighs = 58.7 g

Given quantity = 18.0 kg = 18000 g (1kg=1000g)

58.7 g of Nickel is deposited by 193000 C of electricity

18000 g of Nickel is deposited by = $\frac{193000}{58.7}\times 18000=59182282.8C$ of electricity

$Q=I\times t$

where Q= quantity of electricity in coloumbs = 59182282.8C

I = current in amperes = 31.0 A

t= time in seconds = ?

$59182282.8C=31.0A\times t$

$t=1909105.9sec$

(1h=3600 sec)

$t=530hours$

Thus 530 hours are required to plate 18.0 kg of nickel onto the cathode if the current passed through the cell is held constant at 31.0 A

3 0

3 years ago

How does the concentration of a gas in solution change when the partial pressure of the gas above the solution increases?

irakobra [83]

Because the concentration of molecules in the gas phase increases with increasing pressure, the concentration of dissolved gas molecules in the solution at equilibrium is also higher at higher pressures

5 0

2 years ago

Hydroelectric power plants capture the ______________ of falling water to generate electricity. The falling water turns a wheel

LiRa [457]

Answer:

1: energy

2: converts

Kinetic energy is either 3 or 4, those questions are really similar.

3 0

3 years ago

Complete combustion of 2.60 g of a hydrocarbon produced 8.46 g of co2 and 2.60 g of h2o. what is the empirical formula for the h

zubka84 [21]

1 mole of carbon dioxide contains a mass of 44 g, out of which 12 g are carbon.
Hence, in this case the mass of carbon in 8.46 g of CO2:
(12/44) × 8.46 = 2.3073 g
1 mole of water contains 18 g, out of which 2 g is hydrogen;
Therefore, 2.6 g of water contains;
(2/18) × 2.6 = 0.2889 g of hydrogen.
Therefore, with the amount of carbon and hydrogen from the hydrocarbon we can calculate the empirical formula.
We first calculate the number of moles of each,
Carbon = 2.3073/12 = 0.1923 moles
Hydrogen = 0.2889/1 = 0.2889 moles
Then, we calculate the ratio of Carbon to hydrogen by dividing with the smallest number value;
Carbon : Hydrogen
0.1923/0.1923 : 0.2889/0.1923
1 : 1.5
(1 : 1.5) 2
= 2 : 3
Hence, the empirical formula of the hydrocarbon is C2H3

5 0

4 years ago

Plzzz help do your best to answer these questions

vovikov84 [41]

The empirical formula is the simplest formula of a chemical compound.

To find the empirical formula, we take the following steps;

Divide the percentage by mass of each element by its relative atomic mass.
Divide the quotient of each by the lowest value obtained instep 1 above
Write the result of step 2 above as the subscript following each atom.

1) O - 88.10/16, H - 11.190/1

O - 5.5, H - 11.19

O - 5.5/5.5, H - 11.19/5.5

O - 1, H - 2

Empirical formula = OH2

2) C - 41.368/12 H - 8.101/1, N - 32.162/14, O - 18.369/16

C - 3, H - 8, N - 2, O - 1

C - 3/1, H - 8/1 N - 2/1 O - 1/1

C - 3, H - 8, N - 2, O - 1

Empirical formula = C3H8N2O

To obtain the molecular formula where n = number of atoms of each element;

Molecular weight = 174.204 g/mol

[ 3(12) + 8(1) + 2(14) + 16]n = 174

n= 174/88

n = 2 (to the nearest whole number)

Hence, we have;

[C3H8N2O]2

The molecular formula is C6H16N4O2

3) C - 19.999/12, H - 6.713/1, N - 46.646/14, O - 26.641/16

C - 2, H - 7, N - 3, O - 2

C - 2/2, H - 7/2, N - 3/2, O - 2/2

C - 1, H - 4, N - 2, O - 1

Empirical formula - CH4N2O

brainly.com/question/1363167

5 0

3 years ago

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