**Equilibrium Shifts in Chemical Reactions**For each of the following changes at equilibrium, indicate whether the equilibrium shifts in the direction of the products, the reactants, or does not change.**Reaction:**\[ \text{N}_2 (g) + \text{O}_2 (g) + \text{heat} \rightleftharpoons 2\text{NO} (g) \]**Changes:**a. Increasing the temperature – b. Decreasing the volume of the container – c. Adding a catalyst – d. Adding more \(\text{N}_2 (g)\) – **Explanation:**The reaction is given as a reversible reaction where nitrogen gas (\(\text{N}_2\)) and oxygen gas (\(\text{O}_2\)) combine with heat to form nitrogen monoxide (\(\text{NO}\)). Changes in temperature, pressure, and concentration can affect which direction the equilibrium shifts according to Le Chatelier’s Principle. This principle helps predict the response of an equilibrium system to external changes.

The reaction at equilibrium is given by: The forward reaction is endothermic and the reverse reaction is an exothermic reaction.Le Chatelier's principle: This principle is used to predict the effect of a change in conditions on chemical equilibrium. This principle states that when any system at equilibrium for a long period of time is subjected to a change in concentration, temperature, volume, or pressure the system changes to a new equilibrium, and this change partly counteracts the applied change.The effect of given changes at equilibrium is explained in the table below: S.No. Change equilibrium shifts in the direction of explanation a. Increase the temperature The product The forward reaction is endothermic, hence when equilibrium slightly shift to the product the effect of change of temperature is cancelled. b. Decrease the volume of the container does not change The number of gases reactants (two) and the number of gaseous products (two) is the same, hence there is no effect of change of volume c. Adding a catalyst does not change A catalyst increases the rate of both forward and reverses reactions to the same extent, hence there is no effect of the catalyst at equilibrium. d. Adding more N2(g) The product The forward reaction decreases the concentration of reactant hence the effect of the change is cancelled.

Science

Chemistry

1. For each of the following changes at equilibrium, indicate whether the equilibrium shifts in the direction of the product, the reactants, or does not change N, (g) + 0, (g) + heat 2NO (g) a. Increasing the temperature - b. Decreasing the volume of the container c. Adding a catalyst - d. Adding more N2 (g)

1. For each of the following changes at equilibrium, indicate whether the equilibrium shifts in the direction of the product, the reactants, or does not change N, (g) + 0, (g) + heat 2NO (g) a. Increasing the temperature - b. Decreasing the volume of the container c. Adding a catalyst - d. Adding more N2 (g)

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

(please type answer).
N2(g) + 202(g) → 2NO2(g) A chemist added 0.35 mol of nitrogen gas to 0.45 mol of oxygen gas in 1.0 L container. At equilibrium, the concentration of N2 is 0.30 mol/L. 8. The value of equilibrium concentration of NO2(g) is:
Give typed explanation
.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?
Pretend the following reaction is at equilibrium. How will the equilibrium shift if the volume is suddenly increased? N2(g) + 3H2(g) = 2NH3(g) A. shifts to products B. shifts to reactants C. no shifting
What will the concentration of PCl5 be when equilibrium is reestablished after addition of 1.31 g Cl2? PCl5(g) ⇆ PCl3(g) + Cl2(g) Original Equilibrium Mixture: 3.95 g PCl5 4.86 g PCl3 3.59 g Cl2 in a 1.00-L flask. [PCl5] = ? mol/L
Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed? a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases
Oxygen and ozone are allowed to come to equilibrium in the exothermic reaction 203(g) =302(g) Which change will increase the numerical value of the equilibrium constant, K? Periodic Table and Datasheet Select one: O a. adding more O2(g) O b. adding a suitable catalyst O c. decreasing the temperature O d. increasing the volume of the container
4 NH3(g) +5 O2(g) = 4 NO(g) + 6 H,0(g) AH =-904.4 kJ Consider the equilibrium system represented in the reaction above. Will the concentration of NO increase, decrease, or remain the same when the following experimental changes are made: a. NH, is added d. The volume of the container is reduced b. [H,O] is increased e. A catalyst is added c. O, is removed f. The temperature is increased
#4
34.