At a certain temperature, a 17.0-L container holds four gases in equilibrium. Their masses are 3.5 g SO3, 4.6 g SO₂, 11.9 g ₂. and 0.98 g N₂0. What is the value of the equilibrium constant at this temperature for the reaction of SO₂ with N₂O to form SO3 and N₂? Make sure you balance the reaction using the lowest whole-number coefficients. Kc =

At a certain temperature, a 17.0-L container holds four gases in equilibrium. Their masses are 3.5 g SO3, 4.6 g SO₂, 11.9 g ₂. and 0.98 g N₂0. What is the value of the equilibrium constant at this temperature for the reaction of SO₂ with N₂O to form SO3 and N₂? Make sure you balance the reaction using the lowest whole-number coefficients. Kc =

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

At a certain temperature, a 28.0-L container holds four gases in equilibrium. Their masses are 3.5 g SO3, 4.6 g SO₂, 24.5 g N₂, and 0.98 g N₂O. What is the value of the equilibrium constant at this temperature for the reaction of SO₂ with N₂O to form SO3 and N₂? Make sure you balance the reaction using the lowest whole-number coefficients. Kc = x10 TOOLS
At 30 degrees Celsius the Kc for 2CO(g) + O2(g) = 2CO2(g) is 2.24 x 1022. Predict in which direction the reaction will proceed to reach equilibrium, if we start with 55.0 g CO, 95.0 g O2 and 75.0 g CO2 in a 5.0 L vessel.
Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 6.2 mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.5 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K-0 C = ☐ x10 ×
Suppose a 500. mL flask is filled with 1.3 mol of N₂ and 1.4 mol of O₂. The following reaction becomes possible: N₂(g) + O₂(g) → 2NO(g) The equilibrium constant K for this reaction is 7.02 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. M X S
produces N20 and oxygen. Calculate the value of the equilibrium constant K. for the reaction 2 N,O4(g) –2 N,0(g) + 3 O2(g) from the following information: N2(g) + ¿O2(g) =N‚O(g) K¸ = 2.7 × 10-18 N,O4(g) =2 NO;(g) K. = 4.6 × 10-3 N2(g) + 2 O2(g) =2 NO2(g) K. = 1.7× 10-17
Phosgene is a chemical warfare agent first used on soldiers in World War I. It is synthesized according to the following gas-phase equilibrium reaction: CO(g) + Cl, (g) = COCI,(g) Write the equilibrium expression K, for this reaction below. K. = If K. = 0.281 for this reaction, would the product or the reactant be favored at equilibrium? The reactants would be favored. Neither the product nor the reactants would be favored. The product would be favored.
4. The formation of glucose from water and carbon dioxide is an extremely important reaction for life to exist. Plants perform this reaction through the process of photosynthesis, creating the base of the food chain. The UNBALANCED equation is: H₂O (9) CO2 (g) C6H12O6 (s) + O2 (g) At a particular temperature the equilibrium concentrations were found to be: [H₂0] = 7.90x10-2M, [CO₂] = 0.930M, [0₂] =2.40x10-³M. a. Balance the equation. b. Write an expression for Kc- c. Calculate the value of Kc for the reaction at equilibrium.
Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron/iron oxide catalyst. For the reaction: N₂(g) + 3H₂(g) → 2NH3(g) AH -92.22 kJ/mol At 300 °C the equilibrium constant for the reaction is 4.34 x 10-³. a) Is this reaction endothermic or exothermic? b) What effect would the following changes have on the equilibrium position. Write forward, reverse or no change: • Add some more nitrogen gas • Increase the volume of the reaction vessel • Decrease the temperature • Remove some hydrogen gas
What is the CORRECT equilibrium constant expression for the reaction of N2O (g) and O2(g) to produce NO(g)?
The following reaction is known as the water- gas shift reaction: H2(g) + CO2(g) – – CO(g) + H20(g) for which Kc = 1.53 at a temperature of 686 •C. a. Write an equation for Kc for this reaction in terms of the reactant and product concentrations. b. If you start with only 1.50 M of H20 and 1.50 M of CO, what will the equilibrium concentrations of all four substances be? Construct an ICE table and use the value for Кс above. c. What is the value of Kp for this reaction at 686 •C? d. If the reaction were at equilibrium and then CO2 was removed, in what direction would the reaction shift to recover equilibrium?
9.Suppose 1.000 mole of CO and 3.000 mol of Hydrogen are put in a 10.000 L vessel at 1200 K. Determine the equilibrium composition of the reaction mixture if K. = 3.92 for the reaction. CO (g) + 3H₂(g) → CH4(g) + H₂O(g)
Suppose a 250. mL flask is filled with 1.7 mol of NO2, 0.80 mol of CO and 0.70 mol of CO2. The following reaction becomes possible: NO2(g) + CO(g) = NO(g) + CO2(g) The equilibrium constant K for this reaction is 2.90 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.