16.57 For the reaction H₂ (g) + CO₂ (g) H₂O(g) + CO (g) at 700°C, Kc = 0.534. Calculate the number of moles of H₂ that are present at equilibrium if a mixture of 0.300 mole of CO and 0.300 mole of H₂O is heated to 700°C in a 10.0-L container.

A.) The equilibrium constant, K, for the following reaction is 2.90×10-2 at 1.15×103 K.2SO3(g) 2SO2(g) + O2(g)If an equilibrium mixture of the three gases in a 16.3 L container at 1.15×103 K contains 0.431 mol of SO3(g) and 0.309 mol of SO2, the equilibrium concentration of O2 is ______________________ M. ( fill in the blank )     B.) The equilibrium constant, K, for the following reaction is 6.50×10-3 at 298 K.2NOBr(g) 2NO(g) + Br2(g)If an equilibrium mixture of the three gases in a 19.7 L container at 298 K contains 0.433 mol of NOBr(g) and 0.500 mol of NO, the equilibrium concentration of Br2 is_______________________  M. ( fill in the blank)

A mixture of 1.374 g of H2 and 70.31 g of Br2 is heated in a 2.00 L vessel at 700 K. These substances react according to H2 (g) + Br2 (g) 2HBr (g). At equilibrium, the vessel is found to contain 0.566g of H2. Calculate equilibrium concentrations for H2, Br, and HBr.

Sulfuryl chloride, SO2Cl2 , is a compound with very irritating vapors; it is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature, it decomposes to SO2 and Cl2 .   An 1.00-L flask containing 4.93 g of SO2Cl2 is heated to 375 °C. What is the concentration of SO2Cl2 in the system when equilibrium is achieved?

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g)↽−−⇀4C(g)   ?c=2.13×10^25 If, at this temperature, 2.30mol of A and 3.60mol of B are placed in a 1.00 L container, what are the concentrations of A, B, and C at equilibrium? [A]=                                                             M   [B]=                                                             M   [C]=                                                             M

The equilibrium constant K = 53.09 for H2(g) +12(g) 2 HI(g) has been determined at a certain temperature. If 1.00 mol each of H2 and 12 is placed in a 0.500-L flask at that temperature, what are the concentrations of H2, 12, and HI when equilibrium has been achieved? [H₂]= M [12]= M [H0] => M

Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react according to the following reaction. PCI2(g) + Cl2(g) ⇌ PCI5(g) The equilibrium constant for the reaction is Kc = 43.7 at 130 °C. If 0.587 mo/ of phosphorus trichloride is added to 0.423 mol of chlorine in a 1.26-L reaction vessel and allowed to react at this temperature, what is the equilibrium concentration (in mol/L) of chlorine? Report your answer to THREE significant figures.

The equilibrium constant, Kc , for the following reaction is 7.00×10-5 at 673 K.NH4I(s) NH3(g) + HI(g)If an equilibrium mixture of the three compounds in a 4.05 L container at 673 K contains 2.71 mol of NH4I(s) and 0.262 mol of NH3, the number of moles of HI present is  moles. --- The equilibrium constant, Kc, for the following reaction is 6.30 at 723K.2NH3(g) N2(g) + 3H2(g)If an equilibrium mixture of the three gases in a 12.1 L container at 723K contains 0.250 mol of NH3(g) and 0.208 mol of N2, the equilibrium concentration of H2 is  M.

Consider the reaction: 3H2(g)+N2(g)=2NH3(g) If this reaction is at equilibrium and the pressure is decreased, what will happen to the concentration of H2 and NH3?

The following reaction is important in the production of sulfuric acid. 2SO2(g) + O2(g) 2SO3(g) At 627 °C, 0.0291 mol SO2, and 0.0148 mol O₂ are sealed in a 1.50 L reaction vessel. When equilibrium is reached at the temperature of 725 °C, the concentration of SO3 is determined to be 0.0175 M. What is the value of Ke for the reaction? Calculate the Kp for the reaction at 725 °C. (17 pts.)