4.) Consider the reaction below. Reaction: AH (kJ/mole) 2 ICI (g) 17.78 1 (g) Ca (g) 247.551 116.135 223.066 Umole K) Which is the equilibrium concentration of ICI when 0.45 mol l2, 0.45 mol C2, and 2.42 mol ICl are added to a 2.0L flask at 25°C? A. 0.076 M B. 1.36 M C. 1.14 M D. 0.151 M Keywords: reaction quotient, equilibrium constant, initial concentration(s), final concentration(s), RICE table, equilibrium expression, x-variable atration Concepts: Determination of equilibrium conce

4.) Consider the reaction below. Reaction: AH (kJ/mole) 2 ICI (g) 17.78 1 (g) Ca (g) 247.551 116.135 223.066 Umole K) Which is the equilibrium concentration of ICI when 0.45 mol l2, 0.45 mol C2, and 2.42 mol ICl are added to a 2.0L flask at 25°C? A. 0.076 M B. 1.36 M C. 1.14 M D. 0.151 M Keywords: reaction quotient, equilibrium constant, initial concentration(s), final concentration(s), RICE table, equilibrium expression, x-variable atration Concepts: Determination of equilibrium conce

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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4NH3(g) +50₂(g) = 4NO(g) + 6H₂O(g) AH = -1000. kJ K = 1.35 The equilibrium concentrations are [NH3] = 0.20M, [02] = 0.90M, [H2O] = 1.34 M, and [NO] = [?] What is the equilibrium concentration of NO at 25 °C? [NO] M Enter
Consider the following equilibrium: 2NH3 (g) = N2 (g)+ 3H, (g) AG = 34. kJ Now suppose a reaction vessel is filled with 7.65 atm of ammonia (NH,) and 0.884 atm of hydrogen (H,) at 600. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,? In other words, if you said the pressure of NH, will tend to rise, can that O yes be changed to a tendency to fall by adding N,? Similarly, if you said the O no pressure of NH, will tend to fall, can that be changed to a tendency to rise by adding N,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N, needed to reverse it. ||atm Round your answer to 2 significant digits.
A closed 1.00 L system initially containing 0.00200 mol H₂ and 0.00500 mol 1₂ at a given temperature is allowed to reach equilibrium Analysis of the equilibrium mixture shows that the amount of HI present at equilibrium is 0.00371 mol. Calculate the Kc at this temperature for the reaction. State whether the equilibrium is product-favored or reactant- favored at this temperature. H₂(g) +1₂(g) 2H1(g) Kc 31: The equilibrium is product-favored. Kc 31: The equilibrium is reactant-favored. Kc 0.032; The equilibrium is reactant-favored. Kc - 0.032; The equilibrium is product-favored.
Consider the following equilibrium: N2O4(g) 2NO2 (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 2.78 atm of dinitrogen tetroxide (N204) at 710. °C. Answer the following questions about this system: rise x10 fall Under these conditions, will the pressure of N2O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO2? In other words, if you said the pressure of N2O4 will tend to rise, can that be changed to a tendency to fall by adding NO2? Similarly, if you said the pressure of N2O4 will tend to fall, can that be changed to a tendency to rise by adding NO2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm X S
26) Suppose that at a pressure of 1 atm and temperature 300 K, a given material has two possible phases: liquid (L) and solid (S). We start the system with N₁ = 5 moles in the liquid phase and Ng = 9 moles in the solid phase. For these values of pressure and temperature, PL = 5 x 10-21 J • Hs9 x 10-21 J. What is the equilibrium value of NL? a. 9 mol b. 14 mol c. 1.49 mol d. 5 mol e. O mol
Consider the following equilibrium: 2NOC1 (g) → 2NO(g) + Cl₂ (g) AG = 41. kJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) at 878. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl₂ will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. оо rise fall yes no 0 atm x10 X Ś
Chlorine and bromine gases will react with one another according to the following equation Cl₂(g) + Br₂(g) = 2ClBr(g); Kp = 2.25 If the initial pressure at 298 K of the gases are Cl₂ (9) 1.00 atm, Br₂ (g) 1.00 atm and ClBr(g) 1.50 atm, what will happen as the reaction system moves towards equilibrium? Additional Cl₂ (g) will be formed. O cannot be determined from the given data O additional Cl₂ (g) and Br₂ (g) will be formed O additional ClBr(g) will be formed Onothing, the system is at equilibrium 10-2min- inization the con
Write an expression for the equilibrium constant for the formation of two moles of ammonia gas (NH3) from nitrogen and hydrogen in their standard states. e.g. #A <--> #2B, K = {B}#2/{A}# N2(g) + 3 H2(g) <--> 2 NH3(g) K = [ Select ] ["[N2]", "[H2]", "[NH3]"] [ Select ] ["1", "2", "3"] / [ Select ] ["[N2]", "[H2]", "[NH3]"] [ Select ] ["1", "2", "3"] * [ Select ] ["[N2]", "[H2]", "[NH3]"] [ Select ] ["1", "2", "3"]
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
Consider the following equilibrium: 2NH3(g) = N₂ (g) + 3H₂(g) 2 AG = 34. kJ Now suppose a reaction vessel is filled with 7.87 atm of ammonia (NH3) and 1.17 atm of hydrogen (H₂) at 448. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise fall yes no atm x10 X 5
Be sure to answer all parts. The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) = 2NO(g) K = 4.3 x 10-25 2NO(g) + O2(g) == 2NO,(g) K= 6.4 × 10' Determine the value of the equilibrium constant for the following equation at the same temperature: N2(g) + 202(g) = 2NO2(g) K. - x 10 (Enter your answer in scientific notation.)
Consider the following equilibrium: 2NO(g) + Cl₂ (g) 2NOCI (g) AG=-41. kJ Now suppose a reaction vessel is filled with 1.55 atm of chlorine (C1₂). about this system: T Under these conditions, will the pressure of NOCI tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of NOC1 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if said the pressure of NOCI will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits. and 4.77 atm of nitrosyl chloride (NOCI) at 683. °C. Answer the following questions Orise Ofall yes Ono atm O x10 X S