Answered: For the reversible reaction…

For the reversible reaction N2(g)+O2(g) <=> 2NO(g) the concentrations at equilibrium are [N2] = 0.60 M and [O2] = 0.54 M, and K = 2.1 × 10–3. Find [NO] at equilibrium. _________M NO

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 115IP: For the reaction NH3(g)+H2S(g)NH4HS(s) K = 400. at 35.0C. If 2.00 moles each of NH3, H2S, and NH4HS...

See similar textbooks

Related questions

Q: The equilibrium concentration is determined to be [NO2]= 1.05 M and [N2O4]= 2.20 M. a. Write…

Q: The value of Kc = 2.20•10-10 for the equilibrium of the decomposition of phosgene is: COCl2 (g) D…

Q: For this reversible reaction of gases in a sealed glass vessel at a constant temperature Cl2 (g) + 2…

Q: 3. Given the reaction and corresponding equilibrium constant below, if a 1.0 L flask initially…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: At 100 °C, the equilibrium constant for the reactionCOCl21g2 ∆ CO1g2 + Cl21g2 has the value Kc =2.19…

A: For a reversible reaction at any stage other than the equilibrium, the ratio of the products of the…

Q: The K. for 2 SO2 (g) + O2 (g) =2 SO3 (g) is 7.9 * 104. If you set up a vial with 4.0 * 10-2 M SO3,…

A: Reaction Quotient (Qc) is the ratio between the product of the concentration of the products to that…

Q: the equation: 2A(g) + B(s) = 3C(s) + D(g) Which of the following actions will cause the reaction to…

Q: Which is the correct equilibrium constant expression for the following reaction? Fe 20 3 (s) + 3H 2…

A: Equilibrium constant expression can be described as a product of molar concentration of products…

Q: a Suppose the reaction system CH, (9) + 20, (9) CO,(g) + 2H,0(1) has already reached equilibrium.…

A: Ans According to the Le-Chatliers principle If product removed and reactant added reaction shift…

Q: So Consider the reaction [CO.|H3] [CO|[H,O] K. = = 1 (0.125-z)? %3D %3D CO (s) + H2O (g) = CO2 (g) +…

A: The equilibrium reaction given is, => CO (g) + H2O (g) --------> CO2 (g) + H2 (g)…

Q: At a particular temperature, R= 3.0 X 10 for the reaction 2 CO2 (9) = 2 CO(g) + O2(g) If 2.0 moles…

A: Given that, Equilibrium constant of the reaction (Kc) = 3.0 x 10-6 Number of moles of CO2 present…

Q: A 100.-mL reaction vessel initially contains 2.60 × 10–2 mol of NO and 1.30 × 10–2 mol of H2. At…

A: Given information with unit conversion:

Q: For this reaction: 2O2(g) 2CO(g) + O2(g) K equals 2.35 x 10-5 at a particular temperature. If 3.5…

A: Consider the given information is s follows; Initial moles of CO2 = 3.5 mol Volume of the container…

Q: At a particular temperature, K = 4.2x10^-7 for the following balanced reaction: 2CO2(g) → 2CO(g)…

A: First of all we are going to calculate its molarity by dividing moles to its volume then create ICE…

Q: CH, (g) + H,0 (g) 3 H, (g) + CO (g) is brought to equilibrium at some steady temperature: when this…

Q: Consider the reaction shown below: SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) ; ?? = 0.25 If 0.8251 moles of…

A: Given equilibrium is SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) Equilibrium constant, Kc = 0.25 Initial…

Q: 5. Consider the following reaction and equilibrium constant at a given temperature: NH4CI(s) +…

A: FOr the reaction NH4Cl(s) ⇌ NH3(g) + HCl(g) Kc = 3.5 x 10-3 The volume of vessel=2.00 L Moles of…

Q: For the reaction 2 H2 + 02 ---> 2 H20 K = 81 If you start with [H2] = 10 and [02] =10 and [H2O] = 0,…

A: Concept introduction: The chemical equilibrium is a state in which both reactants and products…

Q: Hydrogen iodide decomposes to form hydrogen and iodine, like this: 2 HI(g) - H2(g) + L(g) Also, a…

A: Kc is defined as the ratio of concentration of products and reactants raised by respective powers.

Q: following reaction. PH3BCl3(s) PH3(g) + BCl3(g) (a) Calculate the equilibrium concentrations of…

Q: The equilibrium constant for the following reaction is 21.3 at 367 °C. K= 21.3 at 367 °C CO(g) +…

Q: Reaction: 1 A + 1B → 2C The initial [A] is 1.00 M and [B] is 1.70 M. The equilibrium constant is…

A: The ratio of equilibrium concentration of products to the equilibrium concentration of reactants is…

Q: 0/5 Calculating an equilibrium constant from a heterogeneous... Nitric acid and nitrogen monoxide…

Q: 11. For the reaction! H2 + Cl2 = 2 HCI 5.512:1 If 5.0 mol of H2 and 3.0 mol of Cl2 are placed in a 2…

A: Given: moles of H2 = 5.0 mol moles of Cl2 = 3.0 mol Volume of flask = 2.0 L Equilibrium moles of H2…

Q: The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600K. COCl2(g) CO(g) +…

Q: For the reversible reaction N2 (g) + O2 (g) the concentrations at equilibrium are [N2] = 0.36 Mand…

A: N2(g) + O2(g) <.....> 2NO(g) At equillibrium : [N2] = 0.36 M [O2] = 1.1M K = 2.1×10-3…

Q: The equilibrium constant for the decomposition of NOCl is 33.7 at a certain temperature. If the…

Q: estion 2 nsider the reversible reaction at equilibrium: 2 SO2(g) + O2(g) +2 SO3. a certain…

A: Equilibrium constant expression, Kc = [SO3]2/[O2][SO2]2

Q: A 3L flask is filled with .45 mol SO3, .5 mol SO2, and .2 mol O2 and allowed to reach equilibrium.…

A: From given The reaction is as follows 2SO3 --- 2SO2 + O2 The concentration of SO3 is determined as…

Q: For the chemical equilibrium A + 2B ⇄ 2C, the value of the equilibrium constant, K, is 10. What is…

A: Given: Equilibrium constant (K) for the reaction A+ 2B ⇄ 2C is 10.

Q: The following reaction has an equilibrium constant Kc equal to 3.07 x 10-4 at 24 °C. 2 NOBr (g)…

A: It is given that the Kc for the reaction is 3.07×10-4 and the reaction is given as follows, 2…

Q: Determine the equilibrium concentration of each species for the following reaction:…

A: Given:

Q: 2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g) The system initially contained 0.2500 M NO, 0.1300 M H2, and…

Q: Consider the equilibrium, CO2(g) + H2(g) < ---- > CO(g) + H2O(g). Calculate the equilibrium…

A: Concentration of H2O = 0.46 M Concentration of H2 = 4.54 M Concentration of CO2 = 9.54 M Kc = 0.0049

Q: 5. What is the equilibrium constant expression for the reaction below? C(s) + CO2(g) + 2C12(g) 2…

Q: Consider the following reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g)SO2Cl2(g)⇌SO2(g)+Cl2(g) A reaction mixture…

A: The chemical reaction : SO2Cl2(g) <---> SO2(g) + Cl2(g) Initial [SO2Cl2] = 2.0 × 10-2 M At…

Q: The following diagram represents the equilibrium state for the reaction: Az (8) + 2 B (g) → 2 AB (g)…

A: In the given reaction, all the chemical species that involve in the reaction are in gas phase. So,…

Q: the phosgene dissociation reaction follows the reaction equation: COCl2 (g) -> CO(g) + Cl2(g).…

A: According to La-Chatelier's principal if in an equilibrium reaction condition of equilibrium are…

Q: A 100.-mL reaction vessel initially contains 2.60 × 10–2 mol of NO and 1.30 × 10–2 mol of H2. At…

Q: For the reaction shown below, at a particular time, the following concentrations are obtained: [CO]…

A: 2CO(g) <.....> C(s) + CO2(g) Kc = 7.7×10-15 [CO] = 0.034 M [CO2] = 3.6×10-17 M To determine…

Q: Consider the following reaction in a chemical equilibrium: 2BrNO(g) ~~~ 2NO(g) + Br2(g) what is…

A: According to the Le-Chatelier's principle, if we increases the concentration of reactant in an…

Q: A 100.-mL reaction vessel initially contains 2.60 × 10–2 mol of NO and 1.30 × 10–2 mol of H2. At…

A: The equilibrium constant, Keq for a reaction is given as :

Q: 14) Consider the following gas-phase reaction: C&H6 (g) + 3H2 (g) E→ C¢H12 (g) When 1.00 mole C6H6…

Q: A 100.-mL reaction vessel initially contains 2.60 × 10–2 mol of NO and 1.30 × 10–2 mol of H2. At…

A: The given reaction is: Concentration is defined as moles / litre. Concentration of NO = 2.60×10-2…

Q: Find [NO] at equilibrium

Q: The equilibrium constant, Kc , for the following reaction is 7.00×10-5 at 673 K. NH4I(s) NH3(g) +…

A: Concentration of NH4I ([NH4I]) = No of moles / Volume in L…

Q: Consider the following equilibrium: N204(8) = 2NO2(g) Suppose two different experiments were…

Q: The reaction Pb(s) + Cd2+ (aq) ⇋ Cd(s) + Pb2+ (aq) has K = 1.00 × 10-9 . At a certain point in the…

A: Since the value of ∆G is given by ∆G = ΔG° + RTln(Q) And ΔG° = -RTln(K) since K = 1 X 10-9 and…

Q: 3. Using ICE Table. The reversible reaction: 2SO2 + Oze) 2SO3 has come to equilibrium in a vessel of…

A: Answer-3 ICE table for the given reaction is: According to problem statement, concentration of SO3…

Q: Consider the following reaction: CO(g) + 2H2 (g) = CH3OH(g) The reaction between CO and H2 is…

A: Given information: Initial concentration of CO = 0.29 M Initial concentration of H2 = 0.48 M…

Question

100%

For the reversible reaction

N₂(g)+O₂(g) <=> 2NO(g)

the concentrations at equilibrium are [N₂] = 0.60 M and [O₂] = 0.54 M, and K = 2.1 × 10^–3. Find [NO] at equilibrium.

_________M NO

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

The equilibrium constant (Kc) for this reaction is 5.0 at a given temperature. CO(g)+H2O(g)CO2(g)+H2(g) (a) On analysis, an equilibrium mixture of the substances present at the given temperature was found to contain 0.20 mol of CO, 0.30 mol of water vapor, and 0.90 mol of H2 in a liter. How many moles of CO2 were there in the equilibrium mixture? (b) Maintaining the same temperature, additional H2 was added to the system, and some water vapor was removed by drying. A new equilibrium mixture was thereby established containing 0.40 mol of CO, 0.30 mol of water vapor, and 1.2 mol of H2 in a liter. How many moles of CO2 were in the new equilibrium mixture? Compare this with the quantity in part (a), and discuss whether the second value is reasonable. Explain how it is possible for the water vapor concentration to be the same in the two equilibrium solutions even though some vapor was removed before the second equilibrium was established.
A 0.72-m01 sample of PCl5 is put into a 1.00-L vessel and heated. At equilibrium, the vessel contains 0.40 mol of PCl3(g ) and 0.40 mol of Cl2(g). Calculate the value of the equilibrium constant for the decomposition of PCl5 to PCl3 and Cl2 at this temperature.
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]
For the reaction NH3(g)+H2S(g)NH4HS(s) K = 400. at 35.0C. If 2.00 moles each of NH3, H2S, and NH4HS are placed in a 5.00-L vessel, what mass of NH4HS will be present at equilibrium? What is the pressure of H2S at equilibrium?
Calculate the pressures of NO, Cl2, and NOCI in an equilibrium mixture produced by the reaction of a starting mixture with 4.0 atm NO and 2.0 atm Cl2. (Hint: KP is small; assume the reverse reaction goes to completion then comes back to equilibrium.) 2NO(g)+Cl(g)2NOCl(g)Kp=2.5103
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.