At 25 °C, the reaction 2NH3(8) = N₂(g) + 3H₂(g) has Kc = 2.3x 10⁹. If 0.043 mol NH3 is placed in a 3.27 L container, what will the concentrations of N₂ and H₂ be when equilibrium is established? Make simplifying assumptions in your calculations. Assume the change in NH3 concentration is insignificant if compared to initial value. [N₂1- eTextbook and Media [H₂] = Save for Later M M Attempts: 0 of 15 used Submit Answer

At 25 °C, the reaction 2NH3(8) = N₂(g) + 3H₂(g) has Kc = 2.3x 10⁹. If 0.043 mol NH3 is placed in a 3.27 L container, what will the concentrations of N₂ and H₂ be when equilibrium is established? Make simplifying assumptions in your calculations. Assume the change in NH3 concentration is insignificant if compared to initial value. [N₂1- eTextbook and Media [H₂] = Save for Later M M Attempts: 0 of 15 used Submit Answer

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

Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 5.96 × 104: H₂(g) + Cl₂(g) →2 HCl(g) Use this information to complete the following table. Suppose a 46. L reaction vessel is filled with 1.8 mol of HCI. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 HCl(g) H₂(g) + Cl₂(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 2 H₂(g)+2Cl₂(g) 4 HCl(g) ܢܢ There will be very little H₂ and Cl₂. There will be very little HCI. Neither of the above is true. K = 0 K = 0 x10 X 0/3 ? olo 18 Ar BA
Suppose a 500. mL flask is filled with 1.6 mol of H₂ and 0.30 mol of HI. This reaction becomes possible: H₂(g) + 12₂(g) → 2HI(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 I2. You can leave out the M symbol for molarity. initial change equilibrium H₂ 0 1₂ x 0 HI 0 X S
8) Consider the system below. When equilibrium is restored, how will the number of each type of molecule and the concentration of each substance compare to those before the stress was introduced? Complete the following table using the words "decrease," "same," or "increase." 2 NH,(g) = N,(g) + 3 H,(g) AH = 92.4 kJ/mol Decrease Volume Decrease Temperature N, Equilibrium Concentration Н, NH, N, Equilibrium Number Н, NH,
16
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
Please don't provide handwriting solutions...
Keq from Equilibrium Composition, Variously Expressed. At some temperature, an equilibrium mixture, in a 1.00-L container, involving the chemical system PCI5(g) = PCI3(g) + Cl2(g) is found to contain 5.74x1020 molecules of PCI5, 0.00921 mol of PCI3, and 0.228 g of Cl2. Calculate the equilibrium constant (Keg expressed in terms of the molar concentrations) at this temperature. (No units required.)
Consider the following equilibrium. N2(s) + O2(g) 2 NO(g) At 2300 K, the equilibrium constant K - 1.7 x 10. Suppose that 0.015 mol NO(g), 0.16 mol N, (9), and 0.16 mol O, (9) are placed into a 10.0 L flask and heated to 2300 K. (a) Is the system at equilibrium? If the system is not at equilibrium, in which direction must the reaction proceed to reach equilibrium? The system is at equilibrium. OThe system is not at equilibrium. The reaction must proceed to the left. The system is not at equilibrium. The reaction must proceed to the right (b) Calculate the equilibrium concentrations of all three substances. (Enter unrounded answers.) [02 - [NO M
Suppose a 500. mL flask is filled with 0.50 mol of Cl₂, 1.7 mol of HCl and 0.20 mol of CC14. The following reaction becomes possible: Cl,(g)+CHCI, (g) → HCI(g) +CCI, (g) 4 The equilibrium constant K for this reaction is 0.104 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places.
Enter your answer in the provided box. The equilibrium constant K. for the equation 2H2(g) + CO(g)=CH3OH(g) is 13 at a certain temperature. If there are 2.21 × 102 moles of H2 and 2.33 x 103 moles of CH;OH at equilibrium in a 4.31-L flask, what is the concentration of CO? M
A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: -6 N, (g) + 3 H, (g) = 2 NH3 (g) К, — 3. х 10 He fills a reaction vessel at this temperature with 6.0 atm of nitrogen gas and 3.2 atm of hydrogen gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NH3, using only the yes x10 tools available to you within ALEKS? no If you said yes, then enter the equilibrium pressure of NH, at right. atm Round your answer to 1 significant digit.
Consider the following reaction: N2 (g) + O2 (g) → 2 NO (g), Kc = 0.25 You start the reaction with 14.72 moles of NO (nitrogen monoxide) in a 2.0 L vessel. Calculate the concentration of O2 (in molarity) at equilibrium. (You do not need to solve a quadratic equation to solve this problem.)