What is the the equilibrium constant (Kc) for the reaction below, if the reaction mixture initially contains 0.595 M CH4 and 0.643 M H₂S, and the equilibrium concentration of H₂ was found to be 0.858 M? CH4(g) + 2H2S(g) = CS2(g) + 4H2(g) Your Answer:

At a certain temperature, the reaction: PCl5(g) ⇆ PCl3(g) + Cl2(g) has an equilibrium constant Kc = 6.7E-6.  Calculate the equilibrium concentration of PCl3 if only PCl5 is present initially at a concentration of 0.30 M.  Your answer should have two significant figures.

Part A For the reaction 3H2 (g) + N2 (g) = 2NH3 (g) at 225 °C the equilibrium contant is 1.7 × 102. If the equilibrium mixture contains 0.13 M H2 and 0.018 M N2 , what is the molar concentration of NH3 ? Express your answer to two significant figures and include the appropriate units.

Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this: 3 NO₂(9)+H₂O(1)→2 HNO3(aq) + NO(g) At a certain temperature, a chemist finds that a 4.4 L reaction vessel containing a mixture of nitrogen dioxide, water, nitric acid, and nitrogen monoxide at equilibrium has the following composition: compound amount NO₂ 10.6 g H₂O 138.4 g HNO3 21.8 g NO 19.6 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. с K = [] x10 ×

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 0.60 mol of CO, 0.30 mol of NO and 1.7 mol of CO,. The following reaction becomes possible: NO,(9) + CO(2) = No(g) + CO,(g) The equilibrium constant K for this reaction is 0.953 at the temperature of the flask. Calculate the equilibrium molarity of NO. Round your answer to two decimal places. 0.37 M ?

Use the References to access important values if needed for this question. The equilibrium constant, Kc, for the following reaction is 0.0290 at 1150 K. 2SO3 (g)2SO2(g) + O2(g) If an equilibrium mixture of the three gases in a 19.7 L container at 1150 K contains 0.251 mol of SO3(g) and 0.353 mol of SO2, the equilibrium concentration of O₂ is M. Submit Answer Retry Entire Group 9 more group attempts remaining

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 ?

CO2(g) + H2(g) « H2O(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000 K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured.                                      [H2]  = 0.20 mol/L                                   [CO2]  = 0.30 mol/L                      [H2O] = [CO]  = 0.55 mol/L (a)   What is the mole fraction of CO(g) in the equilibrium mixture? (b)   Using the equilibrium concentrations given above, calculate the value of Kc, the equilibrium constant for the reaction. (c)   Determine Kp in terms of Kc for this system. (d)   When the system is cooled from 2,000 K to a lower temperature, 30.0 percent of the CO(g) is converted back to CO2(g). Calculate the value of Kc at this lower temperature. (e)   In a different experiment, 0.50 mole of H2(g) is mixed with 0.50 mole of CO2(g) in a 3.0-liter reaction vessel at 2,000 K. Calculate the equilibrium concentration, in moles per liter, of CO(g) at this…

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