The following data were collected for a system at equilibrium at a certain temperature. Calculate the equilibrium constant at this temperature for the reaction. ([H2] = 0.1mol/L; [N2] = 1.1 mol/L; [NH3] = 0.0390 mol.L) 3 H2(g) + N2(g) = 2NH3(g)

The following data were collected for a system at equilibrium at a certain temperature. Calculate the equilibrium constant at this temperature for the reaction. ([H2] = 0.1mol/L; [N2] = 1.1 mol/L; [NH3] = 0.0390 mol.L) 3 H2(g) + N2(g) = 2NH3(g)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.2QE: Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium...

See similar textbooks

Related questions

Q: Consider the following reaction N2(g) + 3H2(g) ⇌ 2NH3(g) ΔH°rxn = –92 kJ Which one of…

A: The given reaction is saber process of ammonia formation. This reaction is an exothermic reaction.

Q: Consider the system 4NH:(g) + 30:(g) 2N:(g) + 6H2O(M AH= -1530.4 kJ How will the amount of ammonia…

A: Answer:- This question is answered by using the simple concept of change in the equilibrium…

Q: Why is there only one value of the equilibrium constant for a particular system at a particular…

A: Equilibrium constant is defined as the ratio of product of equilibrium concentrations of products to…

Q: The reaction 3 O2(g) - 2 O3 (g) has ΔH = +285 kJ/mol. Does the equilibrium constant for the…

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

Q: Determine if the following system is at equilibrium. If not, in which direction will the system need…

Q: Hydrogen sulfide is a pollutant found in natural gas. Following its removal, it is converted to…

Q: 2NO(g) + Cl2(g) ⇄ 2NOCl(g) Kp = 1.4 x 107 0.60 atm NO and 0.70 atm Cl2 are placed in a…

A: Given: Kp = 1.4 × 107 Pressure of NO = 0.60 atm Pressure of Cl2 = 0.70 atm

Q: While ethanol (CH,CH,OH) is produced naturally by fermentation, e.g. in beer- and wine-making,…

Q: Consider the reaction and the value of its equilibrium constant: S2C12(g) + Cl2(g) → 2SCI2(g) Keq =…

A: The equilibrium constant is represented by Keq. and the reaction quotient is Q If Q= Keq the…

Q: system is allowed to once again reach equilibrium. PCI5(g) PCI3(g) + Cl2(g) K= 5.01×10² at 523 K (a)…

Q: Consider the following system at equilibrium where AH° = 10.4 kJ, and K. = 1.80x10-2, at 698 K. %3D…

A: Given: ∆H° = 10.4 KJ Kc = 1.80 × 10-2 Tempreture = 698 K Reaction: 2HI(g) <=> H2(g) + I2(g)…

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

A: The question is based on the concept of equilibrium. It involves application of Le-chatelier…

Q: How can the pressure of water vapor be increased in the following equilibrium?H2 O(l) ⇌ H2 O(g)…

A: Consider the given reaction,

Q: For a reaction PCl5(g) PCl3(g) + Cl2(g) ∆H ̊ = 87.9 kJ in which direction will the equilibrium…

Q: The equation below shows a reaction at equilibrium. What happens to the equilibrium if the…

A: Given reaction : 2NO2(g) <====> N2O4(g) + 58.8 KJ Here , heat energy 58.8 KJ is on product…

Q: Consider the following reaction at equilibrium. What effect will decreasing the temperature have on…

Q: Which one of the following equilibrium reactions is not affected by a change in pressure? H2(g) +…

A: In this question we have to tell the effects on equilibrium by changing in pressure.

Q: Calculate the reaction quotient and determine the direction in which each system will proceed to…

A: Given- 2SO3(g)<->2SO2(g)+O2(g) Kp=6.5atm P(SO2)=1.00atm P(O2)=1.130atm P(SO3)=0.25atm

Q: Consider the following reaction: N2 (g) + 3H2 (g) ⟷⟷ 2NH3 (g) An equilibrium mixture of this…

A: Given that : Concentration of H2 = 7.38 M Concentration of N2 = 2.46 M Concentration of NH3 = 0.166…

Q: The equilibrium of a system cannot be disrupted. O True O False

Q: Which one of the following equilibrium reactions is not affected by a change in pressure? O H2(g) +…

A: By increasing the pressure, equillibrium shift in that direction which has less number of moles of…

Q: equilibrium

Q: Enough NO2 gas is injected into a cylindrical vessel to produce a partial pressure, PNO2, of 0.900…

A: • Answer : Equilibrium partial pressure of N2O4 is 3.24 atm. And equilibrium partial pressure of NO2…

Q: 11. Which of the following things are not applicable to an equilibrium expression iii. Gas ii.…

A: Equilibrium expression :- For a reversible reaction at equilibrium , the ratio of active masses…

Q: A reaction which has reached equilibrium has an equilibrium constant of 0.735. This indicates that,…

A: The equilibrium constant of a reversible chemical reaction determines by the reaction quotient.…

Q: Consider the equilibrium between molecular oxygen and ozone: 3O2(g)>< 2O3(g)…

Q: he following reaction and its equilibrium constant: I2(8) = 2 1(g) Kp = 0.209 %3D A reaction mixture…

Q: In which of the following systems would the number of moles of the substances present at equilibrium…

Q: Consider this equilibrium N,(g)+ 3H,(g) < If some nitrogen gas were injected into this system at…

A: Given that : Pressure and temperature are constant. N2 is added to the system. We need to find which…

Q: Consider the equilibrium: 2SO3(g) 2SO2(g) + O2(g) Kp = 6.5 atm If current pressures are SO2 = 0.40…

Q: - For a certain chemical process, AGº = - 4.955 kJ/mol. What is the equilibrium constant Keq for…

A: The given data: ∆G°= -4.955 kJ/mol R = 8.314 J/mol. K To determine = equilibrium constant Keq

Q: Consider the following system at equilibrium where H° = -108 kJ, and Kc = 77.5 , at 600 K: CO (g) +…

Q: Calculate the reaction quotient and determine the direction in which each of the following reactions…

A: The reaction quotient (Q) measures the relative amount of products and reactants present during a…

Q: Write equilibrium expressions for: N₂(g) + 3H₂(g) + 2NH₂(g) the reaction as written the reverse…

A: Given reaction: N2(g) + 3H2(g) ⇌ 2NH3(g) We have to write the equilibrium expression for: the…

Q: For the reaction, PCl5(g) PCl3(g) + Cl2(g) , Keq = 33.3 at 760°C. Is this system at equilibrium if…

A: Keq is the equilibrium constant. It can be determined by taking the ratio of the concentration of…

Q: Consider the following equilibrium: CO (g) + H2O (g) CO2 (g) + H2 (g) K = 1.6 0.150 mol of CO and…

Q: Consider the reaction: S(s) + 02(g)=S02(g) Write the equilibrium constant for this reaction in terms…

Q: Consider the reaction: S(s) + 02(g) s02(g) Write the equilibrium constant for this reaction in terms…

A: Equilibrium constant is the ratio of equilibrium concentration of products and equilibrium…

Q: The equilibrium constant, Kp, for the reaction PCl5 (g) > PCl3 + Cl2 is 1.26 at 250°C. The reaction…

A: Reaction: Kp = 1.26 at 2500C PCl5 = 0.01 atm PCl3 = 0.2 atm Cl2 = 0.5 atm

Q: I2(g)+Br2(g) --> 2 IBr(g). Kc= 250. the system is charged with 0.0500 M of I2 and Br2. What value…

Q: following equilibrium reaction at 160.00 °C. If 0.420 atm of H2O2(g) is initially present,…

A: Consider the given information is as follows; H2 g + O2g ⇌ H2O2g Kc=7.109…

Q: If Q is greater than K, the system will shift to the right to attain equilibrium. true or false?

A: According to Le Chatelier's principle if a system at equilibrium experience a disturbance by…

Q: H2(g) + I2(g) 2 HI(g) AH=120 kJ e) In which direction will the equilibrium shift (for the first…

A: e) According to the Le- Chatlier principle, when any system at equilibrium is subjected to change in…

Q: 4 b. The following system establishes an equilibrium at 545 K NH₂ (8) + H₂S (8) AND > 0 NH₂HS (s)->…

A: 4) Le Chatelier's principle According to the Le Chatelier's principle when a change in concentration…

Q: Consider the following equation: N2(g) + 2O2(g) + heat 2 NO2(g) In what…

A: if dynamic equilibrium changed by factors like pressure ,temperature,concentration,…

Q: 4. Toluene, C;Hg(1), is an important organic solvent. It is made industrially from…

A: A question based on equilibrium concept, which is to be accomplished.

Q: Consider the reaction: N204(g) 2NO02(g) Write the equilibrium constant for this reaction in terms of…

Q: Given the reaction: PCl3(g) + Cl2(g) ⇌ PCl5(g) Kc = 24.3 Suppose the system at that particular…

A: Given- PCl3+Cl2<->PCl5. Kc=24.3 [PCl3]=0.10M [Cl2]=0.15M [PCl5]=0.55M

Q: Consider the following reaction: 2 NO (g) + O2 (g) ⇌ 2 NO2 (g) Kp = 5.0 x 1012…

Question

3.6

The following data were collected for a system at equilibrium at a certain temperature. Calculate the
equilibrium constant at this temperature for the reaction. ([H,] = 0.1mol/L; [N,] = 1.1 mol/L; [NH3] = 0.0390
mol.L)
3 H2(g) + N2(g) = 2NH3(g)
A K=0.014
B) K=0.14
c) K=4.1
D K=1.4

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

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

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

For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?
What is the pressure of BrCl in an equilibrium mixture of Cl2, Br2, and BrCl if the pressure of CI2 in the mixture is 0.115 atm and the pressure of Br2 in the mixture is 0.450 atm? Cl2(g)+Br2(g)2BrCl(g)KP=4.7102
A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization: 2VCl4V2Cl8 When 6.6834 g VCl4. is dissolved in 100.0 g carbon tetrachloride, the freezing point is lowered by 5.97C. Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm3, and Kf = 29.8C kg/mol for CCl4.)
A common type of reaction we will study is that having a very small K value (K 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be perfomed. However, the math involved when solving equilibrium problems for reactions having small K values (K 1) is simplified. What assumption is made when solving the equilibrium concentrations for reactions with small K values? Whenever assumptions are made, they must be checked for validity. In general, the 5% rule is used to check the validity of assuming x (or 2 x, 3x, and so on) is very small compared to some number. When x (or 2 x. 3x. and so on) is less than 5% of the number the assumption was made against, then the assumption is said to be valid. If the 5% rule fails, what do you do to solve for the equilibrium concentrations?
Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?
Describe a nonchemical system that is in equilibrium, and explain how the principles of equilibrium apply to the system.
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia at equilibrium be affected by (1) removing O2(g)? (2) adding N2(g)? (3) adding water? (4) expanding the container? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.