For the equilibrium system below, which of the following would not result in a decrease in the quantity of H₂(g)? N₂(g) + 3H₂(g) <=====> 2NH3(g) + 94 kJ decreasing the volume of the container decreasing the temperature none of the selections adding some ammonia gas removing some ammonia gas

For the equilibrium system below, which of the following would not result in a decrease in the quantity of H₂(g)? N₂(g) + 3H₂(g) <=====> 2NH3(g) + 94 kJ decreasing the volume of the container decreasing the temperature none of the selections adding some ammonia gas removing some ammonia gas

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

Related questions

Q: Consider the equilibrium below: If 1.5 mol of PCI5 was placed in a 1.0 L container and allowed to…

A: Equilibrium constant Keq for a reaction is defined as the product of the molar concentrations of the…

Q: The equilibrium system shown below was analyzed and the concentrations of H₂(g), 1₂(g) and HI(g),…

A: Equilibrium constant is the product of the molar concentrations of the products, each raised to the…

Q: Which change would cause the equilibrium to shift in the reverse direction? N2(e) + 3 H2(3) #2…

A: An endothermic reaction, heat is absorbed in the reaction, and the value of ΔH is positive. An…

Q: When heat is removed from an exothermic reactions the equilibrium shifts towards the products. True…

A: Answer In exothermic reaction heat released during the process Heat…

Q: Cacog(s) Cao(s) + c02(g) AH"= 178 kimolan The reaction system represented above is at equilibrium.…

A: The change is in amount of reactant or product in an equilibrium is given by Le Chatelier’s…

Q: ammonia. Ammonia is used in the production of fertilizer. The harber process has helped increase…

A: This principle is used to predict the effect of a change in conditions on a chemical equilibrium.…

Q: Choose the equilibrium in which the products are favored by a drop in pressure and the reactants…

A: Le Chatelier's principle: The principle states that the change in concentration, pressure,…

Q: If a reaction is exothermic, and K=100 and Q=1,000, would reactants or products be favored and in…

A: Given: K = 100 Q = 1000 To determine: What direction would equilibrium shift?

Q: Consider the following equilibrium system at 461 K. 2CH2Cl2 (g) 2 CH4 (g) + CC4 (g) If an…

A: Given:[CH2Cl2] = 1.81 x 10-2M[CH4] =3.66 x 10-2M[CCl4] = 1.99 x 10-2M

Q: Consider the following reaction: CO2 (g) + C(s) = 2 CO(g) AH = -588 kJ A 1.0-L container at 1200 K…

A: Answer : Correct option is a ) decreases b) no change Solution : CO2(g) + C(s)…

Q: 1) For the reaction shown below, at a particular time, the following concentrations are obtained:…

Q: Consider the following system at equilibrium where AH° = 111 kJ/mol, and Kc = 6.30, at 723 K. 2 NH3…

A: Answer:When QC=KC, system is at equilibrium.When QC<KC, system is not at equilibrium and in order…

Q: For the Haber process given below, which change will shift equilibrium to the left? N2 (g) + 3 H2…

A: Le-Chatelier’s principle states that any change in pressure, volume, moles or temperature is…

Q: Hydrogen chloride can be made from the reaction of chlorine and hydrogen: Cl2 (g) +H2 (g) → 2HCl…

A: Given data Hydrogen chloride can be made from the reaction of chlorine and hydrogen: Cl2 (g) +H2 (g)…

Q: The following equilibrium C(s) + O₂(g) Set up a table like the one below, and indicate whether…

A: According to the Le-chatelier's principle , when a system is already in equilibrium and a stress is…

Q: What, if anything, would happen if the temperature was increased for an equilibrium reaction mixture…

A: Le Chatelier's principle: This principle is used to predict the effect of a change in conditions on…

Q: 5. N₂(g) + O₂(g) + 2NO(g) Initially, 1.33 mol of nitrogen gas and 2.80 mol of oxygen gas are placed…

Q: Consider the following exothermic reaction, used to obtain lead from its ore: 2PbS (s) + 3O2 (g) +…

Q: The system shown below was analyzed and the concentrations of HF(g)=5.0 mol/L , H2(g)=5.0 mol/L, and…

Q: Refer to the following equilibrium reaction: CaCO3(s) CaO(s) + CO2(g) How would the equilibrium…

Q: For the following equilibrium reaction: 2NO2(g) N2O4(g) + Δ What happens if the pressure of the…

A: Balanced Thermochemical Reaction 2NO2(g) ----> N2O4(g) + Δ If the pressure of the reaction is…

Q: The equilibrium constant is given for one of the reactions below. Determine the value of the missing…

A: Answer The given reaction N2O4(g) --------> 2NO2(g) Kc = 1.46…

Q: Consider the following system at equilibrium. A(aq) = B(aq) AH = +350 kJ/mol What can be said about…

A: The reaction given is, Given: Increase in temperature.

Q: The reaction 3 O2(g)-- H2 O3(g) has ΔH = +285 kJ/mol. Does the equilibrium constant for the reaction…

A: When a reaction proceeds, the reactants convert to products. The amounts of reactants decrease with…

Q: B) Consider the following reaction with a AH° = +190 kJ CH4(g) + 2H₂O(g) CO2(g) + 4H2(g) What will…

A: Le Chaterlier's principle: It states that, if an equilibrium system is subjected to stress then…

Q: The equilibrium constant for the following equilibrium reaction is: 2Hg…

A: Equilibrium constant express relationship between product and reactant of a reaction at equilibrium.…

Q: When the reaction, 2 X(g) + 2 Y(g) = 3 Z(g), reaches equilibrium in an 18-liter container, it is…

A: When the rate of forward reaction is equal to the rate of backward reaction then the reaction is…

Q: Which of the following change will shift the equilibrium to the right for the following reaction?…

A: According to Le chatelier's principle, if a reaction is in equilibrium then if any change is…

Q: For the equilibrium system below, which of the following would result in an increase in the quantity…

A: we have to select the change that results in increase in amount of PCl5

Q: The equilibrium constant is given for two of the reactions below. Determine the value of the missing…

A: If two equilibrium reactions with equilibrium constants K1 and K2 are added together to get a new…

Q: For the equilibrium system below, which action will cause an equilibrium shift to the left? 2 NOCI…

A: According to Le Chatelier principleif a system is in equilibrium is subjected to change of…

Q: Consider the following system at equilibrium at 298 K: 2NO(g) + Br₂(g) 2NOBr(g) + 3.85 kcal Indicate…

A: Le Chatelier principle says if conditions of an equilibrium gets disturbed, the system would try…

Question

For the equilibrium system below, which of the following would not result in a
decrease in the quantity of H₂(g)?
N₂(g) + 3H₂(g) <=====> 2NH3(g) + 94 kJ
decreasing the volume of the container
decreasing the temperature
none of the selections
adding some ammonia gas
removing some ammonia gas

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Introduction

VIEW

Step 2: Explaination

VIEW

Solution

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The equilibrium system shown below was analyzed and the concentrations of H2(g), I2(g) and HI(g), were found, in mol/L, to be 4.2, 3.8, 1.6 respectively. The equilibrium constant must be? H2(g) + I2(g) <=====> 2HI(g) + 65 kJ
Initially 10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2 mol of nitrogen gas is found in the container. The number of moles of ammonia gas at equilibrium would be? 2NH3(g) + 94 kJ <=====> N2(g) + 3H2(g)
Consider this system at equilibrium. A(aq) = B(aq) AH = -350 kJ/mol What can be said about Q and K immediately after an increase in temperature? Q > K because Q increased. = K because neither changed. Q > K because K decreased. Q < K because K increased. О<к because Q decreased. How will the system respond to a temperature increase? shift right shift left no change
The question is attached below
Use the following information to answer the next question Factors that can affect equilibrium I and II III only I, II, and III I. O II only II. III. The factors from the list above that would increase the equilibrium concentration of NO(g) in the system; 4NH3(g) +502 (g) 4NO(g) + 6H₂O(g) AH = -905 kJ while all other variables are held constant are Decreasing the volume Increasing the temperature Adding NH3(g)
For the equilibrium shown below, assess whether the following mixture is at equilibrium. If the mixture is NOT at equilibrium, tell whether the reaction will form more reactant or more products to reach equilibrium. 2 CO2 (g) 2 CO (g) + O2 (g) Kc = 6.4 x 10-7 [CO2] = 5.3 x 10-2 M [CO] = 3.6 x 10-4 M [O2] = 2.4 x 10-3 M
For the equilibrium system below, which of the following would result in an increase in the quantity of H₂(g)? H₂(g) + 12(g) 2HI(g) + 65 kJ ос removing some I₂(g) and removing some HI(g) removing some HI(g) removing some 1₂(g) decreasing temperature removing some HI(g) and decreasing temperature
For the following reaction, calculate all equilibrium concentrations if you start with 1.6 moles of nitrogen dioxide gas in a 4.0 L container. 2NO2(g) <====> N2O4(g) Keq = 1.5 at 250C
Consider the system N2(g) + 3 Cl2(g) 2 NCI3(g) AH = +232 kJ Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by each of the following. decreasing the temperature removing nitrogen trichloride gas 1. forward reaction compressing the system at constant temperature 2. reverse reaction adding chlorine gas
Which way would the equilibrium shift if the temperature was decreased for this reaction (AH = -542 kJ)? H₂ (g) + F₂ (g) → 2HF (g) Shift toward reactants Shift toward products Remain the same None of the above