B. Write the balance equation that would give the following equilibrium.[NO2]2Kc =[NO]2 [O2]

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Answered: Write the balance equation that would…

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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1. 1.86 moles of NOCI was placed in a 2 L reaction vessel and found to contain a total of 0.6 mol of nitrogen monoxide (NO) at equilibrium. Calculate the equilibrium concentrations of all other species in the reaction. NOCI NO + Cl
Consider the following reaction at equilibrium in the gas phase: N2 + 3 H2 double arrows 2 NH3 + heat In which direction will the equilibrium shift if the reaction is cooled? Towards reactants Towards products Neither
What is the correct equilibrium constant expression for the balanced reaction shown below? 2 HCl (g) + I2 (s) 2 HI (g) + Cl2 (g)
Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10-4 M. N2(g) + 3H2(g) = 2NH3(g) Ton: N. x10-2 ent (O Pncca waythe chemical system would 5 the vara BI U = E T O Word(s) ------ T T; O Word(s) 5. If the concentration of the product NH3 was increased from 1.0x 10-4 M to 5.6 x 10-3 M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. B I U E T O Word(s)
Given the following equation: NH4 (aq) + NO2 (aq) → N2(g) + 2H2O (1) AH = -122.4 kJ/mol How would decreasing the pressure effect the equilibrium? It would cause the equilibrium to shift to the right, favoring the products or the forward reaction. It would cause the equilibrium to shift to the left, favoring the reactants or the reverse reaction. It would not effect the equilibrium.
Calculate the mass of PCl5, that must be heated in a 1.0L flask at 250 oC in order to produce enough chlorine to give an equilibrium concentration,[Cl2]eq. of 0.20 mol/L? PCl5(g) <——> PCl3(g) + Cl2(g) Kc = 0.480
Using the above equilibrium expressions, calculate the equilibrium constant, K, for the following concentrations: 3. [HCl] = 1.2 x 10-3 M, [O2] = 3.8 x 10-4 M, [H2O] = 5.8 x 10-2 M, [Cl2] = 5.8 x 10-2 M The equilibrium equation: Keq = [Cl2]^2 [H2O]^2 / [HCl]^+ [O2] ) [NH3] = 0.62 M, [H2] = 0.14 M, [N2] = 0.45 M. the equilibrium equation: Keq= [NH3]^-2 / [H2]^3 [N2] [H2] = 0.0045 M, [Cl2] = 0.0045 M, [HCl] = 0.0625 M. the equilibrium equation: Keq= [HCl]^2 / [H2] [Cl 2] [SO2] = 2.00 M, [O2] = 1.50 M, [SO3] = 3.00 M. the equilibrium equation: Keq = [so3]^2/ [so2]^2 [O2] Please answer all the questions to the best of your ability.
Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction? (a) A catalyst is added to the reaction mixture. which will happen? the equilibrium will not shift the equilibrium will shift towards product but keq will not change the equilibrium will shift towards reactant but keq will not change the equilibrium will shift towards product and keq will increase the equilibrium will shift towards reactant and keq will decrease (b) The total pressure of the system is increased by adding a noble gas. (c) Cl2(g) is removed from the system.
Given the UNBALANCED equilibrium equation: A (g) + B2 (g) AB ( g) Which is the correct equilibrium expression? [A]²[B]! Keg = %3D [AB]? [AB]? Keq = [A]² [B]? (AB]? Keq %3D [A]? [B]! [A]*[B]? [AB]? Keq = %3D [AB]! Keq = [A] [B]?
After equilibrium is reached in the reaction of 6.30 g H2 with 150. g I2, analysis shows that the 1.00 L flask contains 64.0 g of HI. How many moles of H2, I2, and HI are present in this equilibrium mixture? What is the Keq for this reaction?
Indicate whether or not product formation increases if the size of the reaction container is decreased for each of the following equilibrium systems. a) 4NH3(g) + 5O2(g) heat + 4NO(g) + 6H2O(g) b) heat + 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g)
Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. which will happen? the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease (b) The reaction mixture is cooled. the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e)…

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Write the balance equation that would give the following equilibrium. [NO2]? Kc = [NO]2 [02]