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Fofino [41]
3 years ago
13

Which one of the following processes produces a decrease in the entropy of the system?a, precipitation of AgCl(s) from Ag+(aq) a

nd Cl−(aq) ions in solutionb. dissolution of LiOH(s) in waterc. melting solid gold into liquid goldd. evaporation of Hg(l) to form Hg(g)e. mixing of two gases into one container SubmitGive Up Continue
Chemistry
1 answer:
Usimov [2.4K]3 years ago
4 0

Answer:  precipitation of AgCl(s) from Ag^+(aq) and Cl^-(aq) ions in solution

Explanation:

Entropy is the measure of randomness or disorder of a system. If a system moves from  an ordered arrangement to a disordered arrangement, the entropy is said to decrease and vice versa.

\Delta S is positive when randomness increases and \Delta S is negative when randomness decreases.

a) precipitation of AgCl(s) from Ag^+(aq) and Cl^-(aq) ions in solution : As ions are getting solidified, entropy decreases.

b) dissolution of LiOH(s) in water: The compounds dissociates into ions, entropy increases.

c) melting solid gold into liquid gold: The randomness increases, entropy increases.

d) evaporation of Hg(l) to form Hg(g) : The randomness increases, entropy increases.

e)  mixing of two gases into one container : The randomness increases, entropy increases.

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Water is known as the universal solvent. One reason water makes a good solvent is because it is composed of polar molecules. Wha
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Explanation:

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2 years ago
Is this an oxidation reaction? Why or why not?
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Oxygen and Oxygen Ionic or Covalent? Defense how do you know
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Read 2 more answers
Aluminum metal reacts with bromine, a red-brown liquid with a noxious odor. The reaction is vigorous and produces aluminum bromi
GuDViN [60]

<u>Answer:</u> The mass of bromine reacted is 160.6 grams.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}        .....(1)

Given mass of aluminium = 18.1 g

Molar mass of aluminium = 27 g/mol

Putting values in equation 1, we get:

\text{Moles of aluminium}=\frac{18.1g}{27g/mol}=0.670mol

The chemical equation for the reaction of aluminium and bromide follows:

2Al+3Br_2\rightarrow 2AlBr_3

By Stoichiometry of the reaction:

2 moles of aluminium reacts with 3 moles of bromine gas

So, 0.670 moles of aluminium will react with = \frac{3}{2}\times 0.670=1.005mol of bromine gas.

Now, calculating the mass of bromine gas, we use equation 1:

Moles of bromine gas = 1.005 moles

Molar mass of bromine gas = 159.81 g/mol

Putting values in equation 1, we get:

1.005mol=\frac{\text{Mass of bromine}}{159.81g/mol}\\\\\text{Mass of bromine}=(1.005mol\times 159.81g/mol)=160.6g

Hence, the mass of bromine reacted is 160.6 grams.

5 0
2 years ago
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