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At a certain temperature, the equilibrium constant K for the following reaction is 1.0: H,(g) + I,(g) = 2 HI(g) Use this information to complete the following table. Suppose a 38. L reaction vessel is filled with 1.0 mol of H, and 1.0 mol of I,. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little H2 and I. There will be very little HI. Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. %3D 2 HI(g) H,(0)+I,(9) What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K =] 2 H,(0)+21,(0) 4 HI(g) 1. Fynlanation Check

Consider the following system at equilibrium where AH° = -18.8 kJ/mol, and Ke = 10.5 , at 350 K. 2 CH2CI2 (g)=CH4 (9) + CCI4 (9) When 0.34 moles of CH2CI2 (g) are removed from the equilibrium system at constant temperature: The value of K l The value of Qe The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. Oremain the same. It is already at equilibrium. The concentration of CH4 will

Hydrogen chloride decomposes to form hydrogen and chlorine, like this: 2 HCl(g) - H2(9) + Cl,(9) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, hydrogen, and chlorine has the following composition: compound concentration at equilibrium HC1 0.49 M H, 1.9M Cl, 0.10M Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. K̟ = 0

1-A mixture of 0.100 mol of NO, 0.0500 mol of H2, and 0.100 mol of H₂O is placed in a 1.00L vessel. The following equilibrium is established: 2NO(g) + 2H2(g) -- N₂(g) + 2H2O(g) At equilibrium [NO] = 0.0620 M. Calculate the equilibrium concentration of H2, N2, H₂O.

The equilibrium constant K. for the reaction H2(g) + Br2(g) == 2HB1(g) is 2.18 × 10° at 730°C. Starting with 3.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium.

At 400 K, an equilibrium mixture of H2, 12, and HI consists of 0.065 mol H2, 0.079 mol 12, and 0.13 mol HI in a 4.50-L flask. What is the value of K, for the following equilibrium? (R= 0.0821 L atm/(K • mol)) 2HI(g) = H2(g) + 12(8) 0.29 8.2 0.039 O 26 3.4

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.

4. What will be the effect of the following change on the given equilibrium system? system change result CH3OH is added to CH(g) +H20() =CH;OH(1) +H2(g) reaction container H2(g) + I2(g) = 2HI(g) an inert gas is added 2H2 (g) + O2 (g) = 2H20 (g) AH = -483.6 kJ/mol of O2 increase in temperature SnO2(g) + 2C(s) = Sn(s) + 2CO2(g) AH = + 360.0 KJ Pressure is decreased N2(g) + 3 H2(g) =2 NH3(g) AH = -92 kJ mol- the solution is cooled some AgNO; is added to the solution AgCl(s) = Ag*(ag) + CF(ag) N2(g) + 3 H2(g) =2 NH3(g) pressure is increased

References Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 688 K: 2HI(g) H2(g) + I½(g) When he introduced HI(g) at a pressure of 4.87 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of I2(g) to be 0.510 atm. Calculate the equilibrium constant, K,, he obtained for this reaction. %3D Submit Answer