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const2013 [10]
3 years ago
15

1. How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through an aqueous solution conta

ining Cr3+ ions for 40.0 minutes?
Chemistry
1 answer:
Paul [167]3 years ago
6 0

ion with charge 3⁺, like Cr³⁺ needs 3 Faradays to plate 1 mole 

Amount of electric charge per mole (faraday's constant) = 96500 C mol¹⁻

Time = 40min = 2400 sec<span>

you have coulombs = amps x sec = 8 x 2400 coulombs </span>

molar mass of Cr = 51.9961g<span>

96500 x 3 coulombs plates 51.9961g Cr 
so 8 x 2400 coulombs gives,</span>

<span>51.9961/(96500 x 3) x 8 x 2400 g Cr = 3.45g Cr </span>

<span>so, 3.45g chromium metal is plated out.</span>

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At constant pressure and temperature, the mole ratio of the gases is equal to their volume ratio (a consequence of Avogadro's law).

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The following analysis just shows that the other options are not right.

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The mole ratio for this reaction is 2 mol C₂H₂ :5 mol O₂.

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The mole ratio is 1 mol C₃H₈ : 5 mol O₂

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The mole ratio is 2 mol C₂H₆ : 7 mol O₂

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