Consider the following reaction:CuS(s) + O2(g) = Cu(s) + SO2(g)A reaction mixture initially contains 7.38 M O2. Determine the equilibriumconcentration of O2 if Kc for the reaction at this temperature is 1.5.Type the numerical value to three significant figures without units.Answer:

Answered: Image /qna-images/answer/ecbdf2ba-36e3-4296-8c36-d2909a672248.jpg

Consider the following reaction: CuS(s) + O2(g) = Cu(s) + SO2(g) A reaction mixture initially contains 7.38 M O2. Determine the equilibrium concentration of O2 if K. for the reaction at this temperature is 1.5. Type the numerical value to three significant figures without units. Answer:

Consider the following reaction: CuS(s) + O2(g) = Cu(s) + SO2(g) A reaction mixture initially contains 7.38 M O2. Determine the equilibrium concentration of O2 if K. for the reaction at this temperature is 1.5. Type the numerical value to three significant figures without units. Answer:

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 250. mL flask is filled with 0.40 mol of H₂ and 1.3 mol of HI. This reaction becomes possible: H₂(g) +1₂(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 H₂. You can leave out the M symbol for molarity. initial cha equilibrium H₂ 0 X 0 1₂ 0 HI 00 믐 X olo 18 Ar
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
Suppose à 250. mL flask is filled with 1.3 mol of CO, 1.8 mol of H,O and 1.6 mol of H,. This reaction becomes possible: co() +H,0(g) =CO,e)+H,(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. CO H,0 Co, H, initial change equilibrium Explanation Check © 2021 McGraw-Hill Education. All Rights Roserved Terms of Use Privacy 1 Ace O Type here to search
Hydrogen and chlorine react to form hydrogen chloride, like this: H,(g) + Cl,(g) 2 HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chloride has the following composition: compound concentration at equilibrium 0.86 M Cl, 0.30 M HC1 1.9 M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0
Use the following information to answer the next question Factors that can affect equilibrium I and II III only I, II, and III I. O II only II. III. The factors from the list above that would increase the equilibrium concentration of NO(g) in the system; 4NH3(g) +502 (g) 4NO(g) + 6H₂O(g) AH = -905 kJ while all other variables are held constant are Decreasing the volume Increasing the temperature Adding NH3(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.
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 500. mL flask is filled with 0.70 mol of CO, 1.7 mol of NO and 1.0 mol of CO,. The following reaction becomes possible: NO, (g) +CO(g)- NO(g) +CO, (g) The equilibrium constant K for this reaction is 5.97 at the temperature of the flask. Calculate the equilibrium molarity of CO. Round your answer to two decimal places. IM Continue MacBook Air
Suppose a 250. mL flask is filled with 0.30 mol of NO and 0.80 mol of NO2. The following reaction becomes possible: NO3(g)+NO(g)<->2NO2(g) The equilibrium constant K for this reaction is 0.717 at the temperature of the flask. Calculate the equilibrium molarity of NO2. Round your answer to two decimal places.
Consider the following exothermic reaction system at equilibrium: N2(g) + 3H2(g) ⇒ 2NH3(g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below: Note: Use I for increase, D for decrease, NC for no change Add N2(g) Remove H2(g) Add NH3(9) Add Ne(g) Increase the temperature (constant P) Decrease the volume (constant T) Add a catalyst Submit NH3 N₂ H2
Help with the following question Please round the answer to 2 decimal places