Question

For the following reaction at equilibrium in a reaction vessel, which one of these changes would...

For the following reaction at equilibrium in a reaction vessel, which one of these changes would cause the I2 concentration to increase? 2NOI(g) ↔ 2NO(g) + I2(g), /\Hºrxn= 30 kJ/mol

A.

Lower the temperature.

B.

Remove some NO.

C.

Remove some NOI.

D.

Compress the gas mixture into a smaller volume.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

p.s if any problem ask in comments and pls do give upvote thanks.

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
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
1) The following reaction was carried out in a 2.25 L reaction vessel at 1100 K:...
1) The following reaction was carried out in a 2.25 L reaction vessel at 1100 K: C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 8.75 mol of C, 14.1 mol of H2O, 3.60 mol of CO, and 8.50 mol of H2, what is the reaction quotient Q? 2) The following reaction was performed in a sealed vessel at 782 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.65M and...
A) The following reaction was carried out in a 2.00 L reaction vessel at 1100 K:...
A) The following reaction was carried out in a 2.00 L reaction vessel at 1100 K: C(s)+H2O(g)⇌CO(g)+H2(g) If during the course of the reaction, the vessel is found to contain 8.00 mol of C, 14.0 mol of H2O, 3.30 mol of CO, and 6.20 mol of H2, what is the reaction quotient Q? B) The following reaction was performed in a sealed vessel at 772 ∘C : H2(g)+I2(g)⇌2HI(g) Initially, only H2 and I2 were present at concentrations of [H2]=3.10M and  [I2]=2.30M....
Given that evaporation is an endothermic process, which of the following sets of changes would cause...
Given that evaporation is an endothermic process, which of the following sets of changes would cause the following system at equilibrium to shift to increase the number of I2 molecules in the gas phase? I2(s) ⇌ I2(g) a. Increasing container volume and increasing temperature b. Increasing container volume and decreasing temperature c. Decreasing container volume and increasing temperature d. Decreasing container volume and decreasing temperature e. Changing volume or temperature will not affect the number of gas molecules present at...
Given that the following reaction is exothermic, which of the following sets of changes would cause...
Given that the following reaction is exothermic, which of the following sets of changes would cause the following system at equilibrium to shift to increase the number of N2O4(g) molecules? 2NO2(g) ⇌ N2O4(g) What observation would indicate that the reaction is at equilibrium in a closed container? a. Increasing container volume and increasing temperature b. Increasing container volume and decreasing temperature c. Decreasing container volume and increasing temperature d. Decreasing container volume and decreasing temperature e. Changing volume or temperature...
Refer to the reaction system C(s) + H2O(g) ↔ CO(g) + H2(g) at equilibrium for which...
Refer to the reaction system C(s) + H2O(g) ↔ CO(g) + H2(g) at equilibrium for which ΔH°rxn = +131 kJ. Assume ideal gas behavior. Predict the direction in which the above equilibrium will shift as a result of the stated change in conditions. a) An increase in the reaction temperature. b) A decrease in the amount of C(s). c) A decrease in the reactor volume. d) An increase in PH2O. e) Addition of N2 gas to the reaction mixture.
How would you change the volume of the reaction container that holds the following reaction in...
How would you change the volume of the reaction container that holds the following reaction in order to increase the yield of SF6? S(s) + 3 F2(g) ↔ SF6(g) 1) Decrease the volume of the container. 2) Increase the volume of the container. 3) Do not change the volume of the container. 4) Cannot be predicted.\ How does an increase in temperature affect the equilibrium concentration of C and the equilibrium constant for the following reaction? 2 A(g) + B(g)...
The reaction below is at equilibrium at a temperature T. There are four possible changes listed....
The reaction below is at equilibrium at a temperature T. There are four possible changes listed. Select all the changes that will shift the equilibrium so as to produce more products                                     MgO(s) + SO3(g) + 95 kJ   <======> MgSO4(s) I – Increase the temperature                II – Increase the volume III – Add more MgO IV – Remove SO3
At a certain temperature the equilibrium constant, K c, equals 0.11 for the reaction: 2 ICl(g)...
At a certain temperature the equilibrium constant, K c, equals 0.11 for the reaction: 2 ICl(g) ↔ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.25 mol of I2 and 0.25 mol of Cl2 are initially mixed in a 2.0-L flask?
1. A team of chemists is studying the following equilibrium, which has the given equilibrium constant...
1. A team of chemists is studying the following equilibrium, which has the given equilibrium constant at a certain temperature: 2 CH4(g) ⇄ C2H2(g) + 3H2(g) Kp = 2. x 10-7 They fill a reaction vessel at this temperature with 11 atm of methane (CH4) gas.  What is the equilibrium pressure of C2H2? 2. Ammonia decomposes to form nitrogen and hydrogen, like this: 2 NH3(g) ⇄ N2(g) + 3 H2(g) An industrial chemist studying this reaction fills a 25.0 L tank...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT