**Chemical Equilibrium and Le Chatelier's Principle**Assume the reaction below is at equilibrium:\[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) + \text{heat} \]**Question**: Which of the following would shift the equilibrium to the left?- A decrease of temperature- An increase in the amount of \(\text{N}_2\)- A decrease in pressure- A decrease in the amount of \(\text{NH}_3\)**Explanation**: This question involves applying Le Chatelier's Principle, which predicts how a change in conditions can affect the position of the equilibrium in a chemical reaction. The reaction shown is the synthesis of ammonia, which is exothermic (releases heat). - **A decrease of temperature** would shift the equilibrium towards the exothermic direction (right), producing more \(\text{NH}_3\).- **An increase in the amount of \(\text{N}_2\)** would shift the equilibrium to the right, favoring the forward reaction.- **A decrease in pressure** would shift the equilibrium towards the side with more moles of gas, which is the left side (reactants), because 1 mole of \(\text{N}_2\) and 3 moles of \(\text{H}_2\) on the left side make a total of 4 moles, compared to 2 moles of \(\text{NH}_3\) on the right side.- **A decrease in the amount of \(\text{NH}_3\)** would also shift the equilibrium to the right, trying to replace the lost \(\text{NH}_3\).**Correct Answer**: A decrease in pressure.

The given reaction is, N2(g)+3H2(g) ↔2NH3(g)+heat The above reaction is exothermic since heat is released during the reaction.In exothermic reaction, increasing pressure and decreasing the temperature will favor to shift the equilibrium in forward direction. Thus, the correct choice of answer is first option. a decrease of temperature.

Science

Chemistry

Assume the reaction below is at equilibrium. N,(g) + 3H,(g) 5 2NH3 (g) + heat Which of the following would shift the equilibrium to the left? O A decrease of temperature O An increase in amount of N2 O A decrease in pressure O A decrease in amount of NH3

Assume the reaction below is at equilibrium. N,(g) + 3H,(g) 5 2NH3 (g) + heat Which of the following would shift the equilibrium to the left? O A decrease of temperature O An increase in amount of N2 O A decrease in pressure O A decrease in amount of NH3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Which of the following changes will move the equilibrium to the right (products) for the following endothermic reaction? NHẠCO2NH2 (S) 2 NH3 (g) + CO2 (g) O Removing CO2 (g) O Adding NH4CO2NH2 (s) Decreasing the pressure Decreasing the volume Adding NH3 (g) Increasing the temperature
5
.Given the reaction at equilibrium: 2 A(g) + 3 B(g) <--> A2B3(g) + heat Which change will not affect the equilibrium concentrations of A(g), B(g) and A2B3(g)? adding more A(g) adding a catalyst increasing the temperature increasing the pressure
Consider the following gas-phase equilibrium reaction: N2(g) + O2(g) 2NO(g); Kc = 4.10 x 10-4 at 2000 degrees C If 8.00 mol of NO is introduced into a 7.00 L container at 2000 degrees C, what is the concentration of NO when equilibrium is reached?
#8
The following reaction is exothermic. Which change will shift the equilibrium to the left? 2502(g) + O2(g) = 2503(g) raising the temperature adding SO3 removing O2 All of these None of these
3. Given the following reaction: N2 + 3H2 2 2NH3 If the equilibrium [N2] is 1.88 M, the equilibrium [NH3] is 6.62 M, and the equilibrium [H2] is 1.15 M, what is the equilibrium constant?
The equilibrium 4 NH3(g) + 4 O2(g) ⇆ 2 N2O (g) + 6 H2O(l) ΔHo = −142 kJ/mol Is established in a sealed container with a piston. Which of the following actions will increase the amount of the products present at equilibrium? I Increasing the volume of the container II Reducing the volume of the container III Removing some of the H2O(l) from the container IV Adding some NH3(g) to the container V Adding N2(g) to the container VI Raising the temperature VII Lowering the temperature
Given the equilibrium reaction A + B C+ D+heat What change in the reaction system will change the value of the equilibrium constant? O an increase in temperature an increase in the concentration of B and D O an increase in the concentration of A and C O an increase in pressure
3H2(g) + N2(g) ⟷⟷ 2NH3(g) + Heat
3NO3 (g) <----> N2O (g) + NO2 (g) What is the equilibrium constant if the concentrations at equilibrium are as follows: [NO3] = 0.060 M, [N2O] = 0.015 M, and [NO2] = 0.025 M?
For the reaction at eqlibrlum: 3Fe(s) - 4H20(g) = Fez04(s) + 4H2(9), removing some of the product, Fe3O4(s), would: Multiple Choice Increase the value of the equilibrium constant, K Decrease the value of the equilibrium constant, K Shift the equilibrium to the right Shift the equilibrium to the left Cause no change