Question

Indicate which direction the reaction at equilibrium should shift under the given conditions for the reaction...

Indicate which direction the reaction at equilibrium should shift under the given conditions for the reaction of PCl3(g) + Cl2(g) ⇌ PCl5(g).

addition of PCl3

addition of Cl2

addition of PCl5

removal of PCl3

removal of Cl2

removal of PCl5

decrease the volume of the container

addition of Ne

Indicate which direction the reaction at equilibrium should shift under the given conditions for the exothermic reaction of H2(g) + CO2(g) ⇌ H2O(g) + CO(g).

addition of CO2

addition of H2O

addition of H2

removal of H2

removal of CO2

removal of CO

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

PCl3(g) + Cl2(g) ⇌ PCl5(g)

Acccording to LeChateliers principle,

  • Addition of any of the reactant shifts the equilibrium to the right
  • Removal of any of the reactant shifts the equilibrium to the left
  • Addition of any of the product shifts the equilibrium to the left
  • Removal of any of the product shifts the equilibrium to the right
addition of PCl3 shifts to the right
addition of Cl2 shifts to the right
addition of PCl5 shifts to the left
removal of PCl3 shifts to the left
removal of Cl2 shifts to the left
removal of PCl5 shifts to the right
  • Decreasing the volume (or, increase in pressure) equilibrium shifts in the direction where there is less number of moles

For the given equilibrium moles of reactant = 2 and moles of product = 1

Thus, decrease in volume shifts the equilibrium to the right.

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
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.
4. How the reaction conditions (T and P) should be changed in order to shift the...
4. How the reaction conditions (T and P) should be changed in order to shift the equilibrium CO (gas) + H2O (gas) CO2 (gas) + H2 (gas) if ΔН0800K = -36.994 KJ/mol.
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
Indicate any changes that a -d will cause for the following reaction initially at equilibrium: C2H4(g)...
Indicate any changes that a -d will cause for the following reaction initially at equilibrium: C2H4(g) + Cl2(g) reverse arrows C2H4 Cl2(g) + heat All 4 questions have the same answers 1-the system shifts in the direction of the reactants 2- the system shifts in the direction of the products 3- the equilibrium position does not change Part A- raise the temperature of the reaction Part B- decrease the volume of the reaction container Part C- add a catalyst Part...
For the endothermic reaction: 2 H2O(g) <--> 2 H2(g) + O2(g) indicate in which direction the...
For the endothermic reaction: 2 H2O(g) <--> 2 H2(g) + O2(g) indicate in which direction the equilibrium shifts when the following stresses are applied to the system or if there is no change in equilibrium. A. Hydrogen is added to the system. B. The partial pressure of water is increased. C. Oxygen is removed from the system. D. The temperature is increased. E. The volume of the container is decreased. F. A catalyst is added. G. Helium is added 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...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are...
please answear each question 1)At equilibrium, ________. a)the rates of the forward and reverse reactions are equal b)the value of the equilibrium constant is 1 c)all chemical reactions have ceased d)the rate constants of the forward and reverse reactions are equal e)the limiting reagent has been consumed 2)The equilibrium-constant expression depends on the ________ of the reaction. a) stoichiometry b) mechanism c) the quantities of reactants and products initially present d) temperature e) stoichiometry and mechanism 3)Given the following reaction...
Consider the following reaction at equilibrium. What effect will reducing the volume have on the system?...
Consider the following reaction at equilibrium. What effect will reducing the volume have on the system? C3H8(g) + 5 O2(g) ⇌ 3 CO2(g) + 4 H2O(l) ΔH° = -2220 kJ The reaction will shift to the left in the direction of reactants. The equilibrium constant will increase. No effect will be observed. The equilibrium constant will decrease. The reaction will shift to the right in the direction of products.
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180×106 at 730°...
The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180×106 at 730° C. Starting with 4.20 moles of HBr in a 17.8−L reaction vessel, calculate the concentrations of H2,Br2, and HBr at equilibrium. 17. The equilibrium constant Kc for the reaction below is 0.00771 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0433 M and [Br] = 0.0462 M, calculate the concentrations of these species at equilibrium. For the reaction...
3. Consider the reaction N2 (g) + O2 (g) ---------> 2 NO (g) + heat The...
3. Consider the reaction N2 (g) + O2 (g) ---------> 2 NO (g) + heat The product is favored a. When the reaction temperature is increased. b. When the volume of the reaction container is reduced. c. When He (g) is added to the reaction. d. When the reaction temperature is lowered. 4. When the temperature of an equilibrium system for the following reaction is increased, CO (g) + H2O (g) --------> CO2 (g) + H2 (g) the reaction shifts...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT