3. Consider the following reaction where Kc = 3900 at 2000 K 2SO2(g) + O2(g) = 250³(g) a Write the equilibrium constant expression b. Write the reaction quotient expression. c. A reaction vessel contains 0.150 M sulfur dioxide, 0 150 M oxygen and 2.000 M sulfur trioxide. Predict the direction the reaction must shift to reach equilibrium.

3. Consider the following reaction where Kc = 3900 at 2000 K 2SO2(g) + O2(g) = 250³(g) a Write the equilibrium constant expression b. Write the reaction quotient expression. c. A reaction vessel contains 0.150 M sulfur dioxide, 0 150 M oxygen and 2.000 M sulfur trioxide. Predict the direction the reaction must shift to reach 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...

See similar textbooks

Similar questions

4. For the equilibrium CH₂(g) + 2H₂S(g) = CS₂(g) + 4H₂(g), the concentrations at equilibrium are [CH4] = 0.0804 M, [H₂S] = 0.0608 M, [CS₂] = 0.0196 M, and [H₂] = 0.0784 M at 1400.0 K. Using the equilibrium constant expression from before, calculate Kc.
Suppose a 500.mL flask is filled with 1.5mol of CO, 1.1mol of H2O and 1.6mol of H2. The following reaction becomes possible: CO(g)+H2O(g)+CO2(g)+H2(g) The equilibrium constant K for this reaction is 0.840 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places.
8. Consider the reaction: CO + 3H2(g) ↔ CH4(g) + H2O(g) At 500 K, the equilibrium constant for this reaction is KP = 2.48 × 10^-3. Suppose we fill a 7.50 L flask with the four gases. When the mixture reaches equilibrium, the flask contains 0.521 g CO, 0.521 g H2, and 9.20 g H2O. How many grams of CH4 are present?
Given the equation 2A(g) 2B(g) + C(g). At a particular temperature, K = 1.6 × 104.If you mixed 5.0 mol B, 0.10 mol C, and 0.0010 mol A in a one-liter container, which direction would the reaction initially proceed? a To the left. b To the right. c The above mixture is the equilibrium mixture. d Cannot tell from the information given. e None of these (A-D).
4. Initially, a mixture of o.200 M NO, o.100 M Hs, O.200 M H.O was permitted to reach equilibrium (initially there was no Na). At equilibrium, the concentration of NO was discovered to be o.o62 M. Determine the value of the equilibrium constant, Ke, for the reaction: 2 NO(g) + 2 H2(g) S N2(g)+2 H20(g)
Help me plsss.. *For the reaction N2(g) + O2(g) ↔ 2 NO(g), Kc = 4.080×10–4 at 2000 K. What is the equilibrium concentration of N2 and O2, for the reaction 2 NO(g) ↔ N2(g) + O2(g) if the initial concentration of NO is 0.1000 M? *Following the problem above, what is the equilibrium constant of the reverse reaction used? *Following the problem above, if the reaction is reduced to decomposition of 1 mole NO, what is the value of the equilibrium constant?
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant K for the following reaction is 924.: CO(g) + H₂O(g) → CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 17. L reaction vessel is filled with 0.75 mol of CO₂ and 0.75 mol of H₂. 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. CO₂(g) + H₂(9) CO(g)+H₂O(g) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. 3 CO(g) + 3H₂O(g) P 3 CO₂(g) + 3H₂(9) There will be very little CO and H₂O. There will be very little CO2 and H₂. Neither of the above is true. K = 0 K = 0 ■ x10 X ? 00. Ar 8.
consider the reaction h2(g) + f2(g) 2hf(g) with the equilibrium constant k = 100. at some temperature. a) how many moles of h2(g) must be mixed with 1.00 moles of f2(g) in a 1.00 I high-pressure flask to produce 1.70 moles of hf(g) once the flask reaches equilibrium?
Consider the equilibrium system described by the chemical reaction below. For this reaction, Kc = 2.1 × 10³ at a certain temperature. If the equilibrium concentrations of H₂ and F₂ are both 0.0021 M, determine the concentration of HF at equilibrium. H₂(g) + F₂(g) ⇌ 2 HF(g) Kc = [x]2 / [0.0021] [0.0021] = 2.1x103 [HF]eq =
N2(g) and O2(g) can exist in equilibrium with NO(g), as shown below. The equilibrium constant at 25.0°C is 4.8 x 10-31. If initially there are 1.35 mol of nitrogen and 0.60 mol of oxygen in a 2.00 L vessel, find the equilibrium concentrations of each species. N2(g) + O2(g) → 2NO(g)
2 A reaction quotient, Q, is calculated to be 3.2 x 10. The equilibrium constant for the same reaction is 5.4 x 10³. Which statement is correct? a The system is at equilibrium. b The concentrations of the products are greater than their concentrations at equilibrium. The system will attain equilibrium by moving to the right. The system will attain equilibrium by moving to the left. More information is needed to determine which statement is correct. C d e
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.)