1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Jlenok [28]
3 years ago
14

Which of the following are true statements about equilibrium systems? For the following reaction at equilibrium: CaCO3(s) ⇌ CaO(

s) + CO2(g) adding more CaCO3 will shift the equilibrium to the right. For the following reaction at equilibrium: CaCO3(s)⇌ CaO(s) + CO2(g) increasing the total pressure by adding Ar(g) will shift the equilibrium to the right. For the following reaction at equilibrium: 2 H2(g) + O2(g) ⇌ 2 H2O(g) the equilibrium will shift to the left if the volume is doubled. For the following reaction at equilibrium: H2(g) + F2(g) ⇌ 2HF(g) removing H2 will increase the amount of F2 present once equilibrium is reestablished. Increasing the temperature of an endothermic reaction shifts the equilibrium position to the right.
Chemistry
1 answer:
Grace [21]3 years ago
4 0

Answer:

The first, third and fourth statements are correct.

Explanation:

1) For the following reaction at equilibrium: CaCO3(s) ⇌ CaO(s) + CO2(g) adding more CaCO3 will shift the equilibrium to the right.

⇒ Le Chatellier says As the CaCO3 concentration is increased, the system will attempt to undo that concentration change by shifting the balance to the right. <u>This statement is true.</u>

<u />

2) For the following reaction at equilibrium: CaCO3(s)⇌ CaO(s) + CO2(g) increasing the total pressure by adding Ar(g) will shift the equilibrium to the right.

⇒ Le chatellier says that if we increase the pressure, the equilibrium will shift to the side with the least number of particles.

Since the molar densities of CaO and CaCO3 are constant, they don't appear in the equilibrium expression. This is why only changes to the pressure (concentration) of CO2 affect the position of the equilibrium.

If the pressure in the container is increased by adding an inert or non-reacting gas, nothing happens to the amounts of CO2, CaO or CaCO3. The added gas won't affect the partial pressure of CO2. <u>This statement is false. </u>

3)For the following reaction at equilibrium: 2 H2(g) + O2(g) ⇌ 2 H2O(g) the equilibrium will shift to the left if the volume is doubled.

⇒ Le Chatellier says if we increase the pressure, the equilibrium will shift to the side with the most particles.

In this case we have 2 moles of H2 and 1 mole of O2 on the left side and 2 mole of H2O on the right side. This means on the left side are more particles. So the equilibrium will shift to the left, so <u>this statement is true.</u>

4) For the following reaction at equilibrium: H2(g) + F2(g) ⇌ 2HF(g) removing H2 will increase the amount of F2 present once equilibrium is reestablished. Increasing the temperature of an endothermic reaction shifts the equilibrium position to the right.

⇒ Le chatellier says if H2 will be removed (this means the left side will get less particles) so the equilibrium will shift to the left, to increase the amount of F2.

⇒Le chatelier says if we increase the temperature of an exotherm reaction , there will be less energy released. The equilibrium will shift to the side of the reactants (the left side).

If we increase the temperature of an endotherm reaction, the equilibrium will shift to the side of the products (the right side). <u>This statement is true.</u>

You might be interested in
Predict whether each of the following bonds is ionic, polar, covalent, or nonpolar covalent:
Gekata [30.6K]

Explanation:

It is known that in order to determine a compound to be ionic, polar, covalent or non-polar covalent it is necessary to determine the electronegativity difference of the combining atoms.

So, when electronegativity difference is from 0.0 to 0.4 then bond formed between the two atoms is non-polar covalent in nature.

When electronegativity difference is greater than 0.4 and less than 1.8 then bond between the two atoms is a polar covalent bond.

When electronegativity difference is 1.8 or greater than the bond formed is ionic in nature.

Electronegativity difference of the given molecules is as follows.

Si-O = (1.90 - 3.44) = 1.54

K-Cl = (0.82 - 3.16) = 2.34

S-F = (2.58 - 3.98) = 1.4

P-Br = (2.19 - 2.96) = 0.77

Li-O = (0.98 - 3.44) = 2.46

N-P = (3.04 - 2.19) = 0.85

Therefore, given compounds are classified as follows.

Si-O, S-F, P-Br, and N-P all have a polar covalent bond. Whereas K-Cl and Li-O are ionic in nature.

7 0
3 years ago
Read 2 more answers
Which process is an example of a physical change?
Lostsunrise [7]

Answer:

The answer is flattening

Explanation:

A physical change is generally something that affects the shape of form of the matter and a chemical change results from a chemical reaction. Flames are caused by chemical reactions, as is rust, and the process of a fruit becoming ripe. Thus, the answer is “flattening”.

4 0
2 years ago
hello fellow men the challenge has officially begun do not answer this for one month (until november endes). okay well i wish yo
scZoUnD [109]

Answer:

I am not a man or boy, I am a girl so therefore I could answer this question before November ends Imao, have a great rest of your day.

Explanation:

5 0
2 years ago
Read 2 more answers
A car travels a constant speed of 60 Km/h for 3 hours what is the total distance the car has traveled?
ohaa [14]

Answer:

180 miles

Explanation:

60 × 3 = 180

[character limit pass]

7 0
2 years ago
How much water (H2O ) would form if 4.04 g of hydrogen (H2) reacted with 31.98 g of oxygen (O2 )?
Norma-Jean [14]

Answer:

Mass = 36 g

Explanation:

Given data:

Mass of water formed = ?

Mass of hydrogen = 4.04 g

Mass of oxygen = 31.98 g

Solution:

Chemical equation:

2H₂ + O₂   →   2H₂O

Number of moles of hydrogen:

Number of moles = mass/molar mass

Number of moles = 4.04 g/ 2 g/mol

Number of moles = 2.02 mol

Number of moles of oxygen:

Number of moles = mass/molar mass

Number of moles = 31.98 g/ 32 g/mol

Number of moles = 1.0 mol

Now we will compare the moles of water with hydrogen and oxygen.

                O₂         :         H₂O

                 1           :           2

                H₂         :         H₂O

                 2          :          2

               2.02       :      2.02

Number of moles of water formed by oxygen are less thus oxygen will limiting reactant.

Mass of water:

Mass = number of moles × molar mass

Mass = 2 mol × 18 g/mol

Mass = 36 g

8 0
2 years ago
Other questions:
  • What are the elements and number of atoms in the compound c6h12o6?
    5·1 answer
  • 4NH3(g) + 3O2(g) --&gt; 2N2(g) + 6H2O(l)
    5·1 answer
  • A) accelerated upward. B) slowed and then stopped. C) moved at a constant velocity. D) increased its speed rapidly.
    14·1 answer
  • An unknown substance has been shown to have strong ionic bonds. Which of the following is most likely a property of this substan
    12·1 answer
  • Does pyridine undergo nucleophilic aromatic substitution reactions? If no, why not. If yes, on what position does the substituti
    14·1 answer
  • Which two properties define the critical point of matter in a phase diagram?
    12·1 answer
  • The water in an aquarium is warmed by a heater located under the gravel in the bottom of the aquarium.
    9·1 answer
  • I guess you didn’t mean what u wrote in that song about meee
    15·2 answers
  • The melting point for a substance will be the same temperature as its
    5·2 answers
  • Helpppppppppppp me pleaseeeeeee<br><br>​
    5·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!