Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.79 at a certain temperature. If a reaction mixture initially contains 0.050 M H,S and 0.050 M SO2, what will the equilibrium concentration of H20 be? 2 H;S(g) + SO2(g) =3 S(s) + 2 H20(g) 2 3 Based on the given values, set up ICE table in order to determine the unknown. 2 H2S(g) + SO2(g) = 3 S(s) + 2 H20(g) Initial (M) Change (M) Equilibrium (M)

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.79 at a certain temperature. If a reaction mixture initially contains 0.050 M H,S and 0.050 M SO2, what will the equilibrium concentration of H20 be? 2 H;S(g) + SO2(g) =3 S(s) + 2 H20(g) 2 3 Based on the given values, set up ICE table in order to determine the unknown. 2 H2S(g) + SO2(g) = 3 S(s) + 2 H20(g) Initial (M) Change (M) Equilibrium (M)

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...

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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.
At a certain temperature, the equilibrium constant K for the following reaction is 0.71: N2(g) + O2(g) =2 NO(g) Use this information to complete the following table. Suppose a 43. L reaction vessel is filled with 1.0 mol of NO. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and 02. There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K =0 2 NO(g) N,(9)+O2(9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = 3 N2(9)+30,(9) 6 NO(g)
Suppose a 250. mL flask is filled with 1.1 mol of Cl2, 0.20 mol of CHCl3 and 2.0 mol of HCl. The following reaction becomes possible: Cl2(g) + CHCl3(g) HCl(g) +CCI4(g) The equilibrium constant K for this reaction is 0.652 at the temperature of the flask. Calculate the equilibrium molarity of HCI. Round your answer to two decimal places. Ом X G
Consider the following equilibrium: 2NOCl (g) <--> 2NO (g) + Cl2 (g) With K = 1.6 x 10-5. 1.00 mole of pure NOCl and 0.964 mole of pure Cl2 are placed in a 1.00 L container. Calculate the equilibrium concentration of Cl2 (g).
Suppose a 500. mL flask is filled with 0.30 mol of SO, and 1.2 mol of SO3. This reaction becomes possible: 2SO, (g) +O,(g) 2SO3 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 O,. You can leave out the M symbol for molarity. so, SO2 O2 initial change equilibrium
At a certain temperature, the equilibrium constant K for the following reaction is 0.0017: CO(g)+ H₂O(g) CO₂(g) + H₂(g) Use this information to complete the following table. Suppose a 27. L reaction vessel is filled with 1.5 mol of CO and 1.5 mol of H₂0. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. CO,(9)+H,(9) CO(g)+H,O(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 2 CO(g) + 2H₂O(g) 2 CO₂(g)+2H₂(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
For the chemical equation 2SO2(g) + NO2(g) 2SO3(g) + NO(g) The equilibrium constant at a certain temperature is 5.50. At this temperature, calculate the number of moles of NO2(g) that must be added to 1.20 mol SO2(g) in order to form 0.80 mol SO3(g) at equilibrium.
Using the general properties of equilibrium constants At a certain temperature, the equilibrium constant k for the following reaction is 9.84 x 101: N,(g) + 0,(g) = 2 NO(g) Use this information to complete the following table. Suppose a 30. L reaction vessel is filled with 0.64 mol of N2 and There will be very little N, and O2. alo 0.64 mol of 0,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K 2 NO(g) N3(9)+Og(9) What is the equilibrium constant for the following reaction? Round your answer to 3 significant digits. K = 3 N,(9)+30,(9) 6 NO(g)
Can you please answer question 2
Consider the following equilibrium If the equilibrium concentration of chlorine and phosphorous trichloride are 0.80 mol/L and 0.70 mol/L, respectively,find the equilibrium concentration of phosphorous pentachloride.
At a certain temperature, the equilibrium constant k for the following reaction is 6.3 x 10*: NO,(g) + CO(g) = NO(g) + CO,(g) Use this information to complete the following table. Suppose a 40. L reaction vessel is filled with 1.1 mol of NO2 and 1.1 mol of Co. What can you say about the composition of the mixture in the vessel at equilibrium? O There will be very little NO2 and CO. There will be very little NO and CO2. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = NO(9)+CO2(9) NO2(9)+CO(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = | 3 NO,(9)+3CO(9) 3 NO(9)+3CO2(9)