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2 years ago

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An electrolytic cell can be used to plate gold onto other metal surfaces. The plating reaction is: Au (aq) e- --> Au(s) Notic

e from the reaction that 1 mol e- plates out 1 mol Au(s). Use this stoichiometric relationship to determine how much time is required with an electrical current of 0.200 amp to plate out 0.400 g Au. The amp is a unit of electrical current equivalent to 1 C / s. (Hint: Recall that the charge of an electron is 1.60 x 10-19 C.)

1 answer:

Dmitriy789 [7]2 years ago

4 0

Answer:

Explanation:

Faraday’s constant can be used to convert the charge (Q) into moles of electrons (n). The charge is the current (I) multiplied by the time

Q = I × t = n × F

Where

Q is charge

I is current = 0.2A

t is time = ?

n is number of mole

F is Faraday constant = 96500C/s

Mass of Au = 0.4 g = 0.0004kg

Molar mass of Au = 197 g/mol

Malar mass = mass / mole

n = 0.4 / 197

n = 2.03× 10^-3 mol

n = 0.00203 mol

t = n × F / I

t = 0.00203 × 96500 / 0.2

t = 979.7 seconds

t = 16.32 minutes.

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Answer:

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Explanation:

Given:

mass of a block, M = 3.6 kg

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(a)

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$F_c=3.6\times (-6)\times\frac{9.8}{7}$

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$W_c= -30.24\times 4.2$

We take -ve sign because the direction of force and the displacement are opposite to each other.

$W_c=-127.008 J$

(b)

Force on the block due to gravity:

$F_g= M.g$

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$F_g=3.6\times 9.8$

$F_g=35.28 N$

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$W_g=F_g\times d$

$W_g=35.28\times 4.2$

$W_g=148.176 J$

(c)

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K.E. = 21.168 J

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$v^2=u^2+2a_d\times d$

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Answer:

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jarptica [38.1K]

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Explanation:

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