Question

Use the reaction, which produces ammonia, to answer the question.
N2(g) + 3H2(g) ⇄ 2NH3(g)
Which change would happen in the system if the concentration of N2 was increased at constant pressure?


The reverse reaction would increase in order to increase the pressure.

The forward reaction would increase in order to increase the pressure.

The reverse reaction would increase to start reducing the concentration of N2.

The forward reaction would increase to start reducing the concentration of N2.

Answer 1

I explained Le Chatelier's Principle for Burger above. Here is the link.
://www.jiskha.com/questions/1883604/use-the-chemical-reaction-to-answer-the-question-ch4-g-h2o-g-energy-co-g
If you don't understand something repost here and bring it to my attention.

Answer 2

i dont understand chemistry at all i usually wouldnt use a website like this but im failing the class and need to pass this assignment

Answer 3

Why is it so hard to just give us the answer and a explanation so we know how to get the answer. Like give us a break

Answer 4

1.N2(g) + 3H2(g) ⇄ 2NH3(g)
Which change would happen in the system if the concentration of N2 was increased at constant pressure?
Answer ->The forward reaction would increase to start reducing the concentration of N2.
2.In which situation can Le Chatelier’s principle be applied?
Answer->It can be applied when a reaction is reversible, and environmental conditions are changed.
3. N2(g) + 3H2(g) ⇄ 2NH3(g) + energy
When this reaction has reached equilibrium, how will it respond when the temperature of the system increases?
Answer->The equilibrium will shift to the left.
4. CH4(g) + H2O(g) + energy ⇄ CO(g) + H2(g)
Which statement best describes the effect of adding more steam to the system?
Answer->Adding steam allows more molecules of the reactants to collide, causing the rate of the forward reaction to increase.
5. CO(g) + H2O(g) ⇄ CO2(g) + H2(g) + energy
Which change to the system would be favorable to the forward reaction?
Answer->an increase in the concentration of CO

Answer 5

Anonymous is 100% correct thanks Anonymous

Answer 6

1. The forward reaction would increase to start reducing the concentration of N2.
2. It can be applied when a reaction is reversible, and environmental conditions are changed.
3. The equilibrium will shift to the left.
4. Adding steam allows more molecules of the reactants to collide, causing the rate of the forward reaction to increase.
5. an increase in the concentration of CO

[quizlet: captncrun]

Answer 7

^^^friendly neighborhood spiderman is 100% correct for LESSON 4
Changing Reaction Rates
just took the quick check quiz thingy

Answer 8

Y’all ain’t going to pass the act if you can’t understand this simple stuff

Answer 9

spider-man is correct 100%

Answer 10

First of all shut up Idio+ and second both anonymous and friendly neighborhood spiderman are correct.

Answer 11

I agree with Idio+, except it's SAT now, and second of all thanks to those who tried to help!

Answer 12

that's implying I'm going to take it Idio+

Answer 13

Anonymous answer for number 2 is wrong it should be
It can be applied when a reaction is reversible, and environmental conditions are KEPT constant. This is because the principle describes how systems respond to change.

Answer 14

oh if your looking for the answers to Equilibrium and Stability Quick Check here you go
1. A system is at equilibrium. Which statement is correct?
Answer- The rate of the forward reaction equals the rate of the reverse reaction.
2. A sample of water is at equilibrium at 100°C. Which statement best describes what will happen if liquid water is added to the system?
Answer- More liquid water molecules will change to water vapor until a new equilibrium is reached.
3. Use the chemical equation to answer the question.
Co(H2O)62+ + 4Cl– + heat ⇄ CoCl42– + 6H2O
Cobalt ions form complex ions with water and chloride. The Co(H2O)62+ ions are pink, and the CoCl42– ions are blue. A scientist creates a solution that is purple at equilibrium. How can the scientist make the solution more pink?
Answer- by adding water (H2O)
4. Use the chemical equation showing the dissolution of sodium bromide in water to answer the question.
NaBr(s) ⇌ Na+(aq) + Br−(aq)
A student adds hydrobromic acid (HBr) to a solution of sodium bromide at equilibrium. How does this change affect the system?
Answer- The additional bromine ions cause the equilibrium to shift to the reactants.
5. A copper complex reacts with ammonia according to the following reaction, where the left side of the reaction is a pale sky-blue color and the right side is dark blue.
Cu(H2O)42+(aq) + 4NH3(aq) ⇄ Cu(NH3)42+(aq) + 4H2O(aq)
Which change to a solution at equilibrium will make the solution darker?
Answer- Removing water (H2O)

Answer 15

Idio+...

In WHAT world is this simple.

Answer 16

@queen
Honestly this stuff is so hard 😭