Macmillan Learning2 NO(g) + O2(g) = 2 NO2(g)Write the equilibrium-constant expression for the reaction shown in terms of [NO], [O, ], and [NO,].Kc, which is sometimes symbolized as K or Keq, denotes that the equilibrium constant is expressed using molar concentrations.For this question, K, means the same thing as K and Keq.K =

Step 1: The given reaction is:2NO(g)+O2(g)⇌2NO2(g)To write the equilibrium-constant expression…

Answered: Macmillan Learning 2 NO(g) + O2(g) = 2…

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...

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5. Consider the following equilibrium system in equilibrium: X2(g) + 2Y(g) = X2Y½(g). AH>0 Draw a graph of REACTION RATE versus time to show the effects of each of the following changes to the equilibrium system after equilibrium_has been re-established. Provide an explanation for your answers as well. a) The reaction reaches equilibrium for the first time after 10s b) More X2Y2 is added to the system after 20s c) A catalyst is added.to the system after 30 s d) the pressure of the system is increased after 40 s
Consider the following reaction. 2 NO, (g) = N,0,(g) When the system is at equilibrium, it contains NO, at a pressure of 0.858 atm, and N,O, at a pressure of 0.0736 atm. The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished? PNO, = 1.716 atm Incorrect PN,0, .1472 %3D atm Incorrect
Suppose a 500. mL flask is filled with 0.50 mol of N, and 0.90 mol of NO. This reaction becomes possible: N,(8) +O,(g) – 2NO(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of N,. You can leave out the Msymbol for molarity. NO initial change equilibrium
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At a certain temperature, the equilibrium constant K for the following reaction is ×2.0510−7 : Br2g + OCl2g BrOCl g+BrClg Use this information to answer the following question. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K= 3Br2 (g) +3OCl2 (g) 3BrOCl (g) +3BrCl (g
In a particular experiment, it was found that when O2(g) and CO(g) were mixed and allowed to react according to the equation 2C0(g) + O2(g) 2CO2(g) the O2 concentration had decreased by 0.036 molL1when the reaction reached equilibrium. How had the concentrations of CO and CO2 changed? Incorrect. [CO] decrease = i ! mol/L Incorrect. [CO2] increase = i mol/L
Write the equilibrium constant expression, K , for the following reaction: (If either the numerator or denominator is blank, please enter 1.) K=
Coal can be used to generate hydrogen gas (a potential fuel) by the following endothemic reaction (heat is on the reactant side of the equation). C (3) + H20 (g) = co (g) + H2 (g) If this reaction mixture is at equilibrium, predict whether each of the following will resuit in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. Part A adding more C to the reaction mixture the formation of additional hydrogen gas the formation of less hydrogen gas O no effect on the quantity of hydrogen gas
Consider the equilibrium system described by the chemical reaction below. Determine the concentration of O, at equilibrium by writing the equilibrium constant expression and solving it. Complete Parts 1-2 before submitting your answer. = 2 H₂O(g) 2 H2(g) + O̟₂(g) 1 2 NEXT At this temperature, the Kc = 2.4 × 103 and the equilibrium concentrations of H2O and H2 are 0.11 M and 0.019 M, respectively. If [x] represents the equilibrium concentration of O2, set up the equilibrium expression for Kc to solve for the concentration. Each reaction participant must be represented by one tile. Do not combine terms. Кс = 2' = 2.4 × 103 > RESET [0.11] [0.019] 2[0.11] 2[0.019] [0.11]² [0.019]² [x] [x]² [2x] [2x]²
At a certain temperature, the equilibrium constant K for the following reaction is 3.1 × 10 : H,(g) + I,(g) = 2 HI(g) Use this information to complete the following table. Suppose a 36. L reaction vessel is filled with 1.7 mol of HI. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little H2 and I2. There will be very little HI. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = 1 2 HI(g) H2(9)+I,(9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = I 2 H,(9)+21½(9) 4 HI(g)
7) N2(g) + 2O2(g) ------> In the endothermic equilibrium reaction of 2NO2(g), how does the equilibrium system change and in which direction does the equilibrium move when the following operations are performed? a) When the volume is increased, b) When the Cl2 concentration is reduced, c) When the temperature is increased,
Write the equilibrium-constant expression for the reaction shown in terms of [SO2], [CO2], [CS2], and [O2]. 2SO2(g)+CO2(g)↽−−⇀CS2(g)+3O2(g) ?c, which is sometimes symbolized as ? or ?eq, denotes that the equilibrium constant is expressed using molar concentrations. For this question, ?c means the same thing as ? and ?eq.

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