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USPshnik [31]
3 years ago
5

Consider the equilibrium system:

Chemistry
1 answer:
Komok [63]3 years ago
5 0

Answer:

removing the Cl₂ as it is formed .

adding more ICl(s) .

removing some of the I₂(s).

Explanation:

<em>Le Châtelier's principle </em><em>states that when there is an dynamic equilibrium, and this equilibrium is disturbed by an external factor, the equilibrium will be shifted in the direction that can cancel the effect of the external factor to reattain the equilibrium.</em>

<em />

<u>1) Decreasing the volume of the container:</u>

  • Decreasing the volume of the container will increase the pressure.
  • When there is an increase in pressure, the equilibrium will shift towards the side with fewer moles of gas of the reaction. And when there is a decrease in pressure, the equilibrium will shift towards the side with more moles of gas of the reaction.
  • The reactants side (left) has no moles of gases and the products side (right) has 1.0 mole of gases.
  • So, increasing the pressure will shift the reaction to the side with lower moles of gas (left side) and so the total amount of Cl₂ produced is decreased.

so, decreasing the volume of the container will decrease the total amount of Cl₂ produced.

<u>2) Removing the Cl₂ as it is formed:</u>

  • Removing Cl₂ gas will decrease the concentration of the products side, so the reaction will be shifted to the right side to suppress the decrease in the concentration of Cl₂ gas by removing and so the total amount of Cl₂ produced is increased.

so, removing the Cl₂ as it is formed will increase the total amount of Cl₂ produced.

<u><em>3) Adding more ICl(s) :</em></u>

  • Adding ICl(s) will increase the concentration of the reactants side, so the reaction will be shifted to the right side to suppress the increase in the concentration of ICl(s) by addition and so the total amount of Cl₂ produced is increased.

so, adding more ICl(s)  will increase the total amount of Cl₂ produced.

<u>2) Removing some of the I₂(s):</u>

  • Removing I₂ gas will decrease the concentration of the products side, so the reaction will be shifted to the right side to suppress the decrease in the concentration of Cl₂ gas by removing and so the total amount of Cl₂ produced is increased.

so, removing some of the I₂(s) will increase the total amount of Cl₂ produced.

<em>the following changes will increase the total amount of of Cl2 that can be produced:</em>

  • removing the Cl₂ as it is formed .
  • adding more ICl(s) .
  • removing some of the I₂(s).
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Consider 80.0-g samples of two different compounds consisting of only carbon and oxygen. One of the compounds consists of 21.8 g
goldenfox [79]

Answer:

  • <u><em>Ratio of the  mass carbon that combines with 1.00 g of oxygen in compound 2 to the mass of carbon that combines with 1.00 g of oxygen in compound 1 = 2</em></u>

Explanation:

First, detemine the mass of oxygen in the two samples by difference:

  • mass of oxygen = mass of sample - mass of carbon

Item                     Compound 1                        Compound 2

Sample                80.0 g                                    80.0 g

Carbon                 21.8 g                                    34.3 g

Oxygen:               80.0 g - 21.8g = 58.2 g         80.0 g - 34.3 g = 45.7 g

Second, determine the ratios of the masses of carbon that combine with 1.00 g of oxygen:

  • For each sample, divide the mass of carbon by the mass of oxygen determined above:

Sample              Mass of carbon that combines with 1.00 g of oxygen            

Compound 1      21.8 g / 58.2 g =  0.375

Compound 2     34.3 g / 45.7 g = 0.751

Third, determine the ratio of the masses of carbon between the two compounds.

  • Divide the greater number by the smaller number:

  • Ratio = 0.751 / 0.375 = 2.00 which in whole numbers is 2
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PH &amp; POH
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Answer:

<h2>4.0 </h2>

Explanation:

The pH of a solution can be found by using the formula

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From the question we have

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We have the final answer as

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Answer:

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Explanation:

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Some important points about combustion are as follows:

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