Question

According to Le Chatelier's principle, which of the following changes will shift the position of equilibrium...

According to Le Chatelier's principle, which of the following changes will shift the position of equilibrium to the left for the rection: N2 (g) <===> 2NH3 (g) + heat

double the concentraion of N2

increase the concentration of H2

decrease the concentration of NH3

triple the temperature

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #2

According to Le Chatelier's principle,

If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change

Triple the temperature woukd shift the equilibrium to the left. The reaction shown is exothermic. So when temperature os increased accroding to the principle conditions to counteract the change will occur and hence equilibrium shifts towards the left.

In all the other options, the concentrations are increased on the LHS and hence equilibirum shifts to the right to counteract it

answered by: anonymous
0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The reaction below is at equilibrium. Use Le Chatelier's principle to predict the effect of adding...
The reaction below is at equilibrium. Use Le Chatelier's principle to predict the effect of adding ammonia gas to the equilibrium reaction mixture. N2(g) + 3H2(g) 2NH3(g) A. The equilibrium position will remain unchanged. B. The equilibrium position will shift to the right. C. The equilibrium position will shift to the left. D. The equilibrium constant will increase. E. All of the nitrogen gas will be used up.
Determine the direction in which equilibrium will be shifted by the following changes. (Answers can be:...
Determine the direction in which equilibrium will be shifted by the following changes. (Answers can be: shift to products, shift to reactants, no change) N2(g) + 3H2(g) ⇌ 2NH3(g) (This reaction is exothermic and requires a catalyst to occur readily.) a. Increasing [N2]   ______________________________________________ b. Increasing pressure ______________________________________________ c. Decrease in temperature ______________________________________________
According to Le Chätelier's principle, for the equilibrium reaction A(g) "equilibrium arrow" 2B(g) ,what will the...
According to Le Chätelier's principle, for the equilibrium reaction A(g) "equilibrium arrow" 2B(g) ,what will the response of the system be if we: 1.removed B from the system? 2.increased the temperature of the system? 3.added an inert gas (such as nitrogen gas)?
Determine how each of the following changes will affect the equilibrium reaction below (shift left, shift...
Determine how each of the following changes will affect the equilibrium reaction below (shift left, shift right, no change) H2O(g) + C(s) ↔ H2(g) + CO(g) ∆H° = 131 kJ a. increasing the temperature b. adding CO c. removing H2 c. removing H e. increasing the volume of the container f. adding more carbon to the reaction
CO2 and H2 are allowed to react until equilibrium is established as follows: CO2(g) + H2(g)...
CO2 and H2 are allowed to react until equilibrium is established as follows: CO2(g) + H2(g) ↔ H2O(g) + CO(g) Which of the following changes will cause the equilibrium position to shift to the right? a. increase in the concentration of H2 b. decrease in the concentration of CO c. decrease in the concentration of CO2 d. more than one correct response e. no correct response
Calculate the original molarity of strontium hydroxide if the pH is 12.30 Define Le Chateliers principle...
Calculate the original molarity of strontium hydroxide if the pH is 12.30 Define Le Chateliers principle For the synthesis of ammonia (Haber process), the equilibrium constant at 500oC is 6.0 x 10-2. Predict the direction the system will shift to reach equilibrium in the following conditions. [NH3]o = 1.0 x 10-3 M [N2]o = 1.0 x 10-5 M [H2]o = 2.0 x 10-3 M
Ammonia gas, NH3 (g), can be prepared according to the equilibrium below (to be called “the...
Ammonia gas, NH3 (g), can be prepared according to the equilibrium below (to be called “the system” henceforth): N2 (g) + 3H2 (g) ⇌ 2NH3 (g) Kc = 1.2 (at 375 0 C); ΔH0 = - 92 kJ A) Please calculate Kp for this equilibrium. B) Please determine Kp for the decomposition of ammonia into its elements C) Please determine the value of Qc given [NH3] = 0.110 M, [H2] = 0.099 M, and [N2] = 10.1 M. D) Please...
For the following reaction at equilibrium, which change would shift the position of equilibrium toward forming...
For the following reaction at equilibrium, which change would shift the position of equilibrium toward forming more products? (Select your answer(s) as there may be more than one.)2NOBr(g) 2NO(g) + Br2(g), ∆Hºrxn = +30 kJ/mol A)Decrease the total pressure by increasing the volume. B)Add NO. C)Remove Br2. D)Raise the temperature. E)Add NOBr
2. At 450°C, ammonia gas will decompose according to the following equation: 2 NH3 (g) ...
2. At 450°C, ammonia gas will decompose according to the following equation: 2 NH3 (g)  N2 (g) + 3 H2 (g) Kc = 4.50 at 475˚C An unknown quantity of NH3 is placed in a reaction flask (with no N2 or H2) and is allowed to come to equilibrium at 475°C. The equilibrium concentration of H2 is then determined to be 0.252 M. Determine the initial concentration of NH3 placed in the flask
Indicate how each of the following will affect the equilibrium concentration of NH3 in the following...
Indicate how each of the following will affect the equilibrium concentration of NH3 in the following reaction: 4NH3(g)+5O2(g)?4NO(g)+6H2O(g)+906kJ Part A adding more O2(g) a. The equilibrium concentration of NH3 will decrease. b. The equilibrium concentration of NH3 will increase. c. The equilibrium concentration of NH3 will not change. Part B increasing the temperature of the reaction a. The equilibrium concentration of NH3 will increase. b. The equilibrium concentration of NH3 will decrease. c. The equilibrium concentration of NH3 will not...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT