At 2000 °C the equilibrium constant for the reaction 2NO(g) = N₂(g) + O2(g) is Ke 2.4 x 10³. ▼ Part A If the initial concentration of NO is 0.175 M, what is the equilibrium concentration of NO? Express your answer to two significant figures and include the appropriate units. -4.8.10² Submit Part B O Value 1 X Incorrect; Try Again; 4 attempts remaining Submit Part C M If the initial concentration of NO is 0.175 M, what is the equilibrium concentration of N₂? Express your answer to two significant figures and include the appropriate units. A Previous Answers Request Answer wwwww ? Units Request Answer 國」? If the initial concentration of NO is 0.175 M, what is the equilibrium concentration of O₂? Express your answer to two significant figures and include the appropriate units.

At 2000 °C the equilibrium constant for the reaction 2NO(g) = N₂(g) + O2(g) is Ke 2.4 x 10³. ▼ Part A If the initial concentration of NO is 0.175 M, what is the equilibrium concentration of NO? Express your answer to two significant figures and include the appropriate units. -4.8.10² Submit Part B O Value 1 X Incorrect; Try Again; 4 attempts remaining Submit Part C M If the initial concentration of NO is 0.175 M, what is the equilibrium concentration of N₂? Express your answer to two significant figures and include the appropriate units. A Previous Answers Request Answer wwwww ? Units Request Answer 國」? If the initial concentration of NO is 0.175 M, what is the equilibrium concentration of O₂? Express your answer to two significant figures and include the appropriate units.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 108CP: Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain...

See similar textbooks

Similar questions

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.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
At 2000 K, experiments show that the equilibrium constant for the formation of water is 1.6 1010. 2H2(g) + O2(g) 2H2O(g) Calculate the equilibrium constant at the same temperature for H2(g)+12O2(g) H2O(g)
Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant expression for the reaction. Call the equilibrium constant K1. (b) Write an equilibrium constant expression for the formation of one mole of B(g) and call the equilibrium constant K2. (c) Relate K1 and K2.
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
In Table 12.1 (←Sec. 12-3a) the equilibrium constant for the reaction ⇋ is given as 4.2 × 1052. If this reaction is so product-favored, why can large piles of yellow sulfur exist in our environment (as they do in Louisiana and Texas)?
7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.
In each of the reactions, how does the equilibrium respond to an increase in pressure? (a) 2SO 2 ( g )+ O 2 ( g ) 2SO 3 ( g ) (b) H 2 ( g )+ I 2 ( g )2HI( g ) (c) 3H 2 ( g )+ N 2 2NH 3 ( g )
The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
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.