At high temperatures iodine molecules can dissociate into iodine atoms. For the reaction I₂(g) ⇌ 2 I･(g) Kc = 1.27 × 10⁻⁴ at 900 °C. A 25.5 g sample of I₂ is placed in a 1.00 L vessel and heated to 900 °C. What will be the molar concentration of iodine atoms, [I･], in the vessel when the system comes to equilibrium?

The equilibrium constant, K. , for the following reaction is 5.10×10-6 at 548 K. NH,CI(s)NH3(g) + HC(g) If an equilibrium mixture of the three compounds in a 5.06 L container at 54S K contains 3.27 mol of NH,Cl(s) and 0.488 mol of NH3, the number of moles of HCI |moles. present is

A chemist is studying the following equilibirum, which has the given equilibrium constant at a certain temperature: 2NO(g) +  Cl2(g)⇌ 2NOCl(g) Kp=2.x10^−1   He fills a reaction vessel at this temperature with 10.atm of nitrogen monoxide gas and 12.atm of chlorine gas. Use this data to answer the questions in the table below. Can you predict the equilibrium pressure of NOCl, yes or no? If yes, then what is the equilibrium pressure of NOCl? Round your answer to 1 significant digit.

At a certain temperature, the equilibrium constant K for the following reaction is 0.0096 : N,(8) + O,(g) – 2 NO(g) Use this information to complete the following table. Suppose a 13. L reaction vessel is filled with 0.89 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. ? O Neither of the above is true. What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 2 NO(9) N,(9)+0,(9) 1, What is the equilibrium constant for the following reaction? Round your answer to 2 significant digits. K = 0 2 N3(9)+20,(9) 4 NO(9) 1.

The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K.PCl5(g) PCl3(g) + Cl2(g)Calculate the equilibrium concentrations of reactant and products when 0.246 moles of PCl5(g) are introduced into a 1.00 L vessel at 500 K. [PCl5] =  M [PCl3] =  M [Cl2] =  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.

At a certain temperature, the equilibrium constant K for the following reaction is 3.1 × 10 : H,(g) + I,(g) = 2 HI(g) Use this information to complete the following table. Suppose a 36. L reaction vessel is filled with 1.7 mol of HI. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little H2 and I2. There will be very little HI. 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 = 1 2 HI(g) H2(9)+I,(9) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. K = I 2 H,(9)+21½(9) 4 HI(g)

The equilibrium constant, K, for the following reaction is 9.52×10 2 at 350 K. CH, (g) + CCI, (g)=2 CH,Cl, (g) Calculate the equilibrium concentrations of reactants and product when 0.310 moles of CH, and 0.310 moles of CCI, are introduced into a 1.00 L vessel at 350 K. [CH ] M [CCL] =D M [CH,Cl, ] = M

The equilibrium constant, Kc, for the following reaction is 1.29×10-2 at 600 K.COCl2(g) CO(g) + Cl2(g)Calculate the equilibrium concentrations of reactant and products when 0.310 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K.

A chemical engineer is studying the following reaction: 2 H₂S(g)+30₂(g) → 2 SO₂(g) +2H₂O(g) At the temperature the engineer picks, the equilibrium constant K for this reaction is 5.0. The engineer charges ("fills") four reaction vessels with hydrogen sulfide and oxygen, and lets the reaction begin. He then measures the composition of the mixture inside each vessel from time to time. His first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time he measures the compositions. reaction vessel A B compound H₂S 0₂ SO2 H₂O H₂S 0₂ SO₂ H₂O H₂S 02 SO₂ H₂O pressure 9.08 atm 1.44 atm 10.07 atm 8.80 atm 8.96 atm 1.26 atm 10.19 atm 8.92 atm 10.40 atm 3.42 atm 8.75 atm 7.48 atm expected change in pressure ↑ increase O decrease ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase ↑ increase O decrease ↑ increase decrease O decrease ↑ increase O decrease ↓ decrease O decrease ↓ decrease O…