Suppose a 250. mL flask is filled with 1.1 mol of SO, and 1.2 mol of SO,. This reaction becomes possible: 250,(2) +0,(g) – 2so; (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 O,. You can leave out the M symbol for molarity. so, so, initial change equilibrium

Suppose a 250. mL flask is filled with 1.1 mol of SO, and 1.2 mol of SO,. This reaction becomes possible: 250,(2) +0,(g) – 2so; (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 O,. You can leave out the M symbol for molarity. so, so, initial change equilibrium

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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Consider the following reaction: 2NH3 (9) N2(g) + 3H₂ (9) = If 0.00148 moles of NH3(g), 0.268 moles of N₂, and 0.643 moles of H₂ are at equilibrium in a 11.7 L container at 932 K, the value of the equilibrium constant, Ke, is
I am confused because I am getting two possible answers one being 10. 6 and the other being 1.38
Suppose a 250. mL flask is filled with 0.60 mol of N₂ and 0.40 mol of O₂. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 9.69 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places. X
Suppose a 500. mL flask is filled with 1.5 mol of SO, and 0.20 mol of SO2. This reaction becomes possible: 2 (3) 2S0, (g) + 0,(g) =2SO3(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 0,. You can leave out the M symbol for molarity. 2 so, 02 so, initial ? change equilibrium olo
Suppose a 250. mL flask is filled with 0.70 mol of H2 and 1.1 mol of 12. The following reaction becomes possible: H2(g) +I2(g) — 2HI(g) =0 The equilibrium constant K for this reaction is 8.37 at the temperature of the flask. Calculate the equilibrium molarity of 12. Round your answer to two decimal places. Ом
Suppose a 250. mL flask is filled with 0.60 mol of SO₂ and 1.0 mol of SO3. This reaction becomes possible: 2SO₂(g) + O₂(g) — 2SO3(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 O₂. You can leave out the M symbol for molarity. initial change equilibrium SO₂ 0₂ 0 X 0 SO₂ 0 010 X Ś
Suppose a 500. mL flask is filled with 0.30 mol of H, and 1.4 mol of HI. This reaction becomes possible: H,(2) +I,(g) = 2HI(s) 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 I,. You can leave out the M symbol for molarity. H, HI initial change equilibrium Continue Submi O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Priva
2. A reaction is represented by this equation: A(aq) + 2B(aq) = 2C(aq) Ke = 1 × 10³ (a) Write the mathematical expression for the equilibrium constant. (b) Using concentrations S1 M, make up two sets of concentrations that describe a mixture of A, B, and C at equilibrium.
Suppose a 500. mL flask is filled with 0.80 mol of I, and 1.0 mol of HI. This reaction becomes possible: H, (g) +1,(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 I,. You can leave out the M symbol for molarity. H, HI initial change equilibrium
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)
Suppose a 250. mL flask is filled with 1.6 mol of I, and 1.3 mol of HI. This reaction becomes possible: H,(g) +I,(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 H,. You can leave out the M symbol for molarity. H, I, HI initial change equilibrium olo X
Suppose a 500. mL flask is filled with 0.10 mol of O, and 1.6 mol of NO. The following reaction becomes possible: N2(g) + 0,(g) =2NO (g) The equilibrium constant K for this reaction is 0.679 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. | M