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
denpristay [2]
3 years ago
14

Which situation would cause the following equilibrium reaction to decrease the formation of the products? 2SO2 (g) + O2 (g) Two

arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2SO3 (g) + Energy
increase the temperature
decrease the volume
increase the pressure
decrease the temperature
Chemistry
2 answers:
vovangra [49]3 years ago
8 0

The given equilibrium reaction is,

2 SO_{2} (g) + O_{2}(g)  2 SO_{3} (g) + Energy

The given reaction is exothermic. So, heat energy will be a product. Therefore, decreasing the temperature (heat energy) would lead to the formation of more products as when the amount of energy which is a product is reduced, there is more room for the products to form.

Increasing the pressure would shift the equilibrium towards that side which has least number of moles of the gaseous substance. Hence, here increasing the pressure would lead to the formation of more products by shifting the equilibrium towards the right side.

Decreasing the volume would make the equilibrium shift towards the least number of moles of the gaseous substance. So, here in this equilibrium decreasing the volume would lead to the formation of more products.

MaRussiya [10]3 years ago
8 0

Answer:  increase the temperature

Explanation: Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

2SO_2+O_2\leftrightharpoons 2SO_3+energy

This is a type of Exothermic reaction because heat is released in the reaction.

Option A: Increase the temperature

If the temperature is increased, so according to the Le-Chatlier's principle , the equilibrium will shift in the direction where decrease in temperature occurs. As, this is an exothermic reaction, forward reaction will increase the temperature. Hence, the equilibrium will shift in the left direction, products will decrease.

Option B: Decrease the volume  and Option C: increase in pressure

If the volume of the container is decreased, the pressure will increase according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease in pressure is taking place. As the number of moles of gas molecules is greater at the reactant side. So, the equilibrium will shift in the right direction, products will increase.

Option D: Decrease the temperature

If the temperature is decreased, so according to the Le-Chatlier's principle , the equilibrium will shift in the direction where increase in temperature occurs. As, this is an exothermic reaction, forward reaction will increase the temperature. Hence, the equilibrium will shift in the right direction, products will increase.

You might be interested in
Using the scientific method, design an experiment to test whether snow in Delaware makes better snowman than in New Jersey. Be s
FrozenT [24]

Answer:

Bro do the experiment and find it out

5 0
2 years ago
How many moles are in 22 grams of neon?
11111nata11111 [884]

Answer:

0.9911 mol

Explanation:

7 0
3 years ago
Most carbon based molecules are classified as
kherson [118]
<span>the answer is organic molecule                                                                  </span>
7 0
3 years ago
Read 2 more answers
If 100 ml of a 0.5 M HCI Solution is diluted with water to 1000ml, what is the new concetration?
Vesna [10]

Answer:

0.05\ \text{M HCl}

Explanation:

V_1 = Initial volume = 100 mL

V_2 = Final volume = 1000 mL

M_1 = Initial concentration = 0.5 M

M_2 = Final concentration

We have the relation

\dfrac{M_1}{M_2}=\dfrac{V_2}{V_1}\\\Rightarrow M_2=M_1\dfrac{V_1}{V_2}\\\Rightarrow M_2=0.5\times \dfrac{100}{1000}\\\Rightarrow M_2=0.05\ \text{M HCl}

The new concentration is 0.05\ \text{M HCl}.

3 0
3 years ago
Which of the following values is measured the LEAST precisely? * 22mL 45.2mL 50mL 100mLchem​
nekit [7.7K]

Answer:

If you're looking at the data as a whole, it would most likely be 100ml.

Explanation: The definition of precise is data close together so 100ml is furthest away from the other recorded numbers

7 0
3 years ago
Other questions:
  • If I added 50 mL of a 1.0 M HCIO2 solution to 50 mL of a 1.0 M NaOH
    5·1 answer
  • What are weak bonds that allow flexibility in enzymes
    8·1 answer
  • The molar mass of an unknown gas was measured by an effusion experiment. It was found that it took 60 s for the gas to effuse, w
    8·1 answer
  • Please help me with this it’s for my bell ringer
    11·1 answer
  • Concerning Boyle's Law, if you had a gas at a pressure of 101 kPa and decreased the volume of the container holding the gas to o
    7·1 answer
  • Consider the addition of HBr to 2-pentene. Indicate the re
    11·1 answer
  • 2 HCl + 1 Zn -&gt; 1 H2 + ZnCl2 what type of reaction is this
    11·1 answer
  • How much volume (in cm3) is gained by a person who gains 12.3 lb of pure fat?
    11·1 answer
  • For 20 points.... answer this
    13·2 answers
  • 21.041gMg - 21.00gMg/ 24.31 (gmg/ mol Mg)
    12·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!