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Feliz [49]
3 years ago
12

A particular voltaic cell operates with the reaction: Zn(s)+Cl2(g)--->Zn^2+(aq)+2Cl^-(aq) giving a cell potential of .853 V.

Calculate the amount of energy liberated from the cell when 20.0g of zinc metal is consumed?
Chemistry
1 answer:
nadya68 [22]3 years ago
3 0

Answer:

The amount of energy liberated will be 49.38 J.

Explanation:

The amount of energy liberated (gibbs free energy) can be calculated using the following equation:

ΔG° = -nFε

n: amount of moles of electrons transfered

F: Faraday's constant

ε: cell potential

20.0 g of Zn is equal to 0.30 mol.

Two electrons are transfered during the reaction.

Therefore, n = 2x0.30 ∴ n = 0.60

ΔG° = - 0.60 x 96.485 x 0.853

ΔG° = 49.38 J

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natita [175]

Answer :

(a) The density of mercury is, 13.6 g/ml

(b) The mass of 120.0 ml of mercury is, 1632 grams

Explanation :

(a) Now we have to calculate the density of mercury.

<u>Given :</u>

Volume of mercury = 25.0 ml

Mass of mercury = 340.0 g

Formula used :

\text{Density of mercury}=\frac{\text{Mass of mercury}}{\text{Volume of mercury}}

\text{Density of mercury}=\frac{340.0g}{25.0ml}=13.6g/ml

Therefore, the density of mercury is, 13.6 g/ml

(b) Now we have to calculate the mass of 120.0 ml of mercury.

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So, 120.0 ml of mercury has mass = \frac{120.0ml}{25.0ml}\times 340.0g=1632g

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3 0
3 years ago
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Answer:

A

Explanation:

7 0
3 years ago
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Write the complete balanced equation for the reaction between iron (III) oxide (Fe2O3) and water (H2O). You do not need to make
Alina [70]
Fe2O3+3H2O->2Fe(OH)3
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Silver metal can be prepared by reducing its nitrate, AgNO3 with copper according to the following equation:
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%yield = 88.5%

<h3>Further explanation</h3>

Given

Reaction

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Solution

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% yield = (actual/theoretical) x 100%

%yield = 71.5/80.784 x 100%

<em>%yield = 88.5%</em>

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2 years ago
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timofeeve [1]

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