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Alekssandra [29.7K]
3 years ago
13

Aluminum has a density of 2.70 g/cm3. what would be the mass of a sample whose volume is 10.0 cm3?

Chemistry
1 answer:
anastassius [24]3 years ago
3 0
Hey there!

Density = 2.70 g/cm³

Volume = 10.0 cm³

Therefore:

Mass = density *  volume

Mass = 2.70 * 10.0

Mass = 27.0 g
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How many formula units are present in 40.0 grams of Cu2S?
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What is the energy change associated with 1.5 mole of D being formed? 
AleksandrR [38]

Answer:

–36 KJ.

Explanation:

The equation for the reaction is given below:

2B + C —› D + E. ΔH = – 24 KJ

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This can be obtained as illustrated below:

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3 0
2 years ago
Flag question
Ghella [55]

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3 years ago
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Use calc to determine whether it is possible to remove 99.99% Cu2 by converting it to Cu(s) in a solution mixture containing 0.1
inessss [21]

Answer:

it is possible to remove 99.99% Cu2 by converting it to Cu(s)

Explanation:

So, from the question/problem above we are given the following ionic or REDOX equations of reactions;

Cu2+ + 2e- <--------------------------------------------------------------> Cu (s) Eo= 0.339 V

Sn2+ + 2e- <---------------------------------------------------------------> Sn (s) Eo= -0.141 V

In order to convert 99.99% Cu2 into Cu(s), the equation of reaction given below is needed:

Cu²⁺ + Sn ----------------------------------------------------------------------------> Cu + Sn²⁺.

Therefore, E°[overall] = 0.339 - [-0.141] = 0.48 V.

Therefore, the change in Gibbs' free energy, ΔG° = - nFE°. Where E° = O.48V, n= 2 and F = 96500 C.

Thus, ΔG° = - 92640.

This is less than zero[0]. Therefore,  it is possible to remove 99.99% Cu2 by converting it to Cu(s) because the reaction is a spontaneous reaction.  

7 0
3 years ago
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