The reaction for the formation of nitrosyl chloride was studied at 25 °C. 2NO (g) + Cl2 (g) + 2NOCI (g) For a-d, show all calculations and explain your answers. a. Pressures at equilibrium were tabulated as: PNOCI = 1.2 atm, PNo = 5.0E-2 atm, Pc12 = 3.0E-1 atm. Calculate the value of K, for this reaction at 25 °C. These are three scenarios which are about the same reaction at 25 °C, each with different conditions. b. If 1.0 atm NOCI(g) was added to an evacuated (empty) container, would a reaction occur? If so, in which direction would the reaction proceed? If 1.0 atm each of NOCI(g), NO(g), and Cl2(g) were added to an evacuated (empty) container at this temperature, would a reaction occur? If so, in which direction would the reaction proceed? C. www

The reaction for the formation of nitrosyl chloride was studied at 25 °C. 2NO (g) + Cl2 (g) + 2NOCI (g) For a-d, show all calculations and explain your answers. a. Pressures at equilibrium were tabulated as: PNOCI = 1.2 atm, PNo = 5.0E-2 atm, Pc12 = 3.0E-1 atm. Calculate the value of K, for this reaction at 25 °C. These are three scenarios which are about the same reaction at 25 °C, each with different conditions. b. If 1.0 atm NOCI(g) was added to an evacuated (empty) container, would a reaction occur? If so, in which direction would the reaction proceed? If 1.0 atm each of NOCI(g), NO(g), and Cl2(g) were added to an evacuated (empty) container at this temperature, would a reaction occur? If so, in which direction would the reaction proceed? C. www

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...

See similar textbooks

Similar questions

If Q is the reaction quotient and K is the equilibrium constant, when the constant is at equilibrium what is true? A. Q<K B. Q^2=K C. Q>K D. K^2=QE. Q=K
Consider the equilibrium N₂O4(g) = 2NO₂(g). At 500 °C, the equilibrium mixture contained 3.86 M nitrogen dioxide gas. Calculate the equilibrium concentration of dinitrogen tetroxide if Kc at this temperature is 0.847. Provide your answer to two places after the decimal and without units. Type your answer...
7. Please refer to the attached photo. Thank you!!
( give handwritten clean ans
The following reaction was initiated with NOCl(g), with a partial pressure of NOCl(g) = 0.66 atm. The reaction achieved equilibrium at 25⁰C where equilibrium partial pressure for NOCl(g) : (?????(?) ) = 0.33 atm. Calculate the KC value for this reaction. 2 NOCl(g) ⇌ 2 NO(g) + Cl2(g) A) 3.3 × 10-4 B) 0.165 C) 3.3 D) 6.74 × 10-3 E) 0.0042 atm
At 35°C, K = 1.8 x 10-5 for the reaction 2 NOCI(g) 2 NO(g) + Cl₂ (g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.4 moles of pure NOCI in a 2.0-L flask. M Q F4 [NOCI] [NO] = M [Cl₂] = M b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask F5 Submit Answer [NOCI] [NO] = [C12] M c. 2.0 mole of NOC1 and 1.0 mole of Cl2 in a 1.0-L flask [NOCI] = M [NO] = [C12] Show Hint A 6 = F6 = = & 7 Retry Entire Group K F7 8 DII FB M M M M 9 more group attempts remaining ( 9 DD F9 0 F10 Previous F11 Next Save and Exit F12
8
For the reaction in a sealed container at a constant temperature,2NO(g)+Br2(g)2NOBr(g)the initial concentrations are 5.35 M NO, 8.70 M Br2, and no NOBr. At equilibrium, [NOBr] = 1.73 M. Calculate the value of K under the reaction conditions.K =
At a given temperature, the equilibrium constant K, for the reaction below is 2.68×10¯³. 2s0,(g) +02(g) 2so, (g) What is the value of the equilibrium constant for each of the following reactions at that temperature? so,) + 0,) – so,() 250, (2). - 250, (g) + 0,(g) so, )
At 25°C, K= 0.090 for the reaction H20(g) + Cl20(9) = 2 HOCI(9) Calculate the concentrations of al1 species at equilibrium for each of the following cases. a. 1.0 g H20 and 2.0 g Cl2 0 are mixed in a 1.0-L flask. [H2O] =| M [CL,0] = M [HOC1] = M b. 1.2 mole of pure HOCI is placed in a 2.0-L flask. [H2O] = M [Cl20] = M %D [HOCI] = M
At 35°C, K = 2.1 × 10-5 for the reaction 2 NOCI(g) – 2 NO(g)+ Cl2 (9) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 3.6 moles of pure NOCI in a 2.0-L flask [NOCI] = M [NO] = M [Cl2] = M b. 1.0 mole of NOCI and 1.0 mole of NO in a 1.0-L flask [NOCI] = M [NO] = M [Cl2] = M c. 2.8 mole of NOCI and 1.0 mole of Cl2 in a 1.0-L flask [NOCI] = M %3D [NO] : M %3D [Cl2] = M
Consider the following reaction: PCI5(g) – PCI3(g) + Cl2(g) K, = 23.6 at 500 K a. Calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PPCI, = 0.560 atm and PpCl, = 0.500 atm. b. If more chlorine is added after equilibrium is reached, how will the concentrations of PCls and PC13 change?