Suppose a 250. mL flask is filled with 0.80 mol of H₂O, 0.50 mol of CO₂ and 1.7 mol of H₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂ (g) + H₂(g) The equilibrium constant K for this reaction is 9.79 at the temperature of the flask. Calculate the equilibrium molarity of CO₂. Round your answer to two decimal places. M X S

Suppose a 250. mL flask is filled with 0.80 mol of H₂O, 0.50 mol of CO₂ and 1.7 mol of H₂. The following reaction becomes possible: CO(g) +H₂O(g) CO₂ (g) + H₂(g) The equilibrium constant K for this reaction is 9.79 at the temperature of the flask. Calculate the equilibrium molarity of CO₂. Round your answer to two decimal places. M X S

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

Suppose a 500. mL flask is filled with 1.7 mol of Cl₂, 1.1 mol of CHCl3 and 1.3 mol of HCl. The following reaction becomes possible: Cl₂(g) + CHCl3 (g) → HC1(g) +CC14 (g) The equilibrium constant K for this reaction is 9.41 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. 10999
Suppose a 250. mL flask is filled with 0.70 mol of Cl₂ and 1.1 mol of HCI. The following reaction becomes possible: H₂(g) + Cl₂(g) 2HCl(g) The equilibrium constant K for this reaction is 0.288 at the temperature of the flask. Calculate the equilibrium molarity of Cl₂. Round your answer to two decimal places. M 1
I am confused because I am getting two possible answers one being 10. 6 and the other being 1.38
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.
Suppose a 250. mL flask is filled with 0.70 mol of NO₂, 0.20 mol of NO and 1.9 mol of CO₂. The following reaction becomes possible: NO₂ (g) + CO (g) NO(g) + CO₂(g) The equilibrium constant K for this reaction is 0.715 at the temperature of the flask. Calculate the equilibrium molarity of NO₂. Round your answer to two decimal places.
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.
Suppose a 250. mL flask is filled with 1.6 mol of Br₂, 0.70 mol of OC12 and 0.50 mol of BrCl. The following reaction becomes possible: Br₂(g) + OC1₂(g) → BrOC1 (g) + BrCl(g) The equilibrium constant K for this reaction is 2.87 at the temperature of the flask. Calculate the equilibrium molarity of Br₂. Round your answer to two decimal places. M Ś
Suppose a 250. mL flask is filled with 1.1 mol of NO3 and 2.0 mol of NO. The following reaction becomes possible: NO3(g) + NO(g) → 2NO,(g) The equilibrium constant K for this reaction is 8.88 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places.
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.
Suppose a 500. mL flask is filled with 1.5 mol of H₂ and 1.2 mol of Cl₂. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) The equilibrium constant K for this reaction is 3.45 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M Ś
Suppose a 250. mL flask is filled with 1.4 mol of CO, 1.9 mol of H₂O and 1.0 mol of CO₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) 2 The equilibrium constant K for this reaction is 9.28 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. M X Ś ?
Suppose a 500. mL flask is filled with 1.9 mol of Cl₂, 1.5 mol of CHC13 and 0.60 mol of HC1, The following reaction becomes possible: Cl₂(g) + CHC1₂(g) → HC1(g) +CC1₂(g) The equilibrium constant K for this reaction is 9.28 at the temperature of the flask. Calculate the equilibrium molarity of HC1. Round your answer to two decimal places. OM X