3. The equilibrium constant for the following reaction is Kp = 5.60 x 104 at 350 °C.2SO2(g) + O2(g) = 2SO3(g)a) Write the equilibrium equation.b) The equilibrium constant is very large (56000). Does equilibrium favor the products or thereactants?c) The reaction occurs when high sulfur coal is burned. In once example, the initial pressure of SO₂is 0.350 atm and O₂ is 0.762 atm. Calculate Qp. What does Qp tell about the direction of theequilibrium.d) The product of this reaction, SO3(g) reacts with water (H₂O(g)) to form a product which is thesource of acid rain. Write this reaction. Find the equilibrium constant for this reaction.

Predicting the extent of reaction: The magnitude of the equilibrium constant gives an idea relative…

3. The equilibrium constant for the following reaction is Kp = 5.60 x 104 at 350 °C. 2SO2(g) + O₂(g) = 2SO3(g) a) Write the equilibrium equation. b) The equilibrium constant is very large (56000). Does equilibrium favor the products or reactants? c) The reaction occurs when high sulfur coal is burned. In once example, the initial presse is 0.350 atm and O₂ is 0.762 atm. Calculate Qp. What does Qp tell about the direction a equilibrium. d) The product of this reaction, SO3(g) reacts with water (H₂O(g)) to form a product which source of acid rain. Write this reaction. Find the equilibrium constant for this reaction.

3. The equilibrium constant for the following reaction is Kp = 5.60 x 104 at 350 °C. 2SO2(g) + O₂(g) = 2SO3(g) a) Write the equilibrium equation. b) The equilibrium constant is very large (56000). Does equilibrium favor the products or reactants? c) The reaction occurs when high sulfur coal is burned. In once example, the initial presse is 0.350 atm and O₂ is 0.762 atm. Calculate Qp. What does Qp tell about the direction a equilibrium. d) The product of this reaction, SO3(g) reacts with water (H₂O(g)) to form a product which source of acid rain. Write this reaction. Find the equilibrium constant for this reaction.

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

Consider the following equilibrium reaction: N2(g) + O2(g) = 2 NO(g) Kp = 3.67 x 101 at T = 75°C 2.50 atm of N2(g) and 2.50 atm of O2(g) are placed in a 3.00L flask and allowed to reach equilibrium. a) Write the Kp expression for this reaction. b) Determine the equilibrium partial pressures of each reactant and product. (BOX YOUR FINAL ANSWER.) c) Once the reaction is at equilibrium and the volume of the container is increased to 5.50 L, in which direction, if any, will the reaction proceed? Explain your answer.
Equilibrium mixture in a 2.50 L flask at 250 °C in the reaction PCI3(g) + Cl₂(g) →PCI5(g); It contains 0.105 g PCI5, 0.220 g PCI3, and 2.12 g Cl₂. What is the value of (a) Kc and (b) Kp for this reaction at 250 °C? P: 31 g/mol; CI: 35.5 g/mol
Carbon tetrachloride can be produced by the following reaction: CS2(g)+3 Cl2 (g)S, Cla (s) +CCL, (g) Suppose 1.20 mol of CS2 and 3.60 mol of Cl2 were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.61 mol of CC14. Calculate Kc at the unknown temperature.
Consider the equilibrium system described by the chemical reaction below. At equilibrium, a sample of gas from the system is collected into 5.00 L flask. The flask is found to contain 8.62 g of CO, 2.60 g of H2, 43.0 g of CH4, and 48.4 g of H:O at 320.0 °C. What are the values of Kc and Kp for this reaction? CH:(g) + H2O(g) = CO(g) + 3 H2(g) 1 2 NEXT > Based on the given data, set up the expression for Kc and then evaluate it. Do not combine or simplify terms.
In the reaction below, 5 atm of H2 and 1 atm of Cl2 were placed into a 1.00 L flask and allowed to react: H2(g) + Cl2(g) <=> 2 HCl(g) Given that Kp at 900 K is K = 16, calculate the equilibrium pressure of HCl and give to 2 decimal places.
Please don't provide handwritten solution ...
8. Consider the equilibrium reaction: N2(g) + O2(g) = 2 NO(g) Kp 4.10 x 10³ at 2000°C a) If 1.00 atm of nitrogen gas and 1.00 atm of oxygen gas is mixed with 0.10 atm of nitrogen monoxide in a 500.0 mL container at 2000°C, in which direction will the reaction proceed to reach equilibrium? Show all work to justify your answer. b) What is the concentration of each gas when equilibrium is reached at 2000°C? Show all your work. Equilibrium Partial Pressures: PN₂ = Po₂ = 1.02 atm and PNO = 0.07 atm Use PV = nRT Answer: Equilibrium Concentrations: [N₂] = [0₂] = 5.47 x 10-3 mol/L and [NO] = 4 x 10+ M
A gas mixture consisting of 1.05 Atm of SO3 and 0.425 Atm of O2 was placed in a container and after the equilibrium 2SO2 (g) + O2 (g) ⇄ 2SO3 (g) was established, the total pressure was 1.62 Atm. What is the equilibrium constant, Kp?
An empty steel container is filled with 3.10 atm of H₂ and 3.10 atm of F2. The system is allowed to reach equilibrium. If Kp = 0.450 for the reaction below, what is the equilibrium partial pressure of HF? H₂ (g) + F₂ (g) → 2 HF (g)
Please don't provide handwritten solution...
Consider the equilibrium system below. For this reaction, Kp = 205. If the equilibrium partial pressure of Cl2 is 0.050 atm and the partial pressure of NOCl is 0.095 M what is the equilibrium partial pressure of NO? 2 NO (g) + Cl2 (g) <-> 2 NOCl (g)