14). For the reaction below: 2NH3(g) = N2(g) + 3H2(g) We initially mixed 1 M of N2 gas and 2 M of H2 gas in a 1.0 L sealed flak and allowed the reaction to reach equilibrium. When equilibrium is established what are the terms representing each of the concentration of the gases? Or, another word, what are the terms at the Line E? + 3H2(g) 2 + 2x b. 2NH3(g) = N2(g) + 3H2(g) 1 + x 2NH3(g) = N2(g) 1 + x а. Line E: -2x 2 + x Line E: -2x + ЗН-(9) 2 - 3x d. c. Line E: 2x 2NH3(g) = N½(g) 1- x 2NH3(g) = N2(g) + 3H2(g) 2 - 2x 3H2(g) 2 - 3x 1-x Line E: 2x 2NH3(g) = N½(g) + 1 - 2x е. Line E: 2x

What is the equilibrium concentration of BCl3 if a solid sample of PH3BC13 is placed in a 0.250 L closed vessel at 80.0 °C and decomposes until equilibrium is reached? Assume that there is solid present at equilibrium. At 80.0 °C, Kc = 1.87 x 10-³ for the reaction: PH3BC13(s) ⇒ PH3(g) + BCl3(g) Provide your answer in M, without units, and use the correct number of significant figures. 534.8

Iron(III) oxide and hydrogen react to form iron and water, like this: Fe,O3(s)+3 H2(9)–→2 Fe(s)+3 H,O(g) At a certain temperature, a chemist finds that a 4.5 L reaction vessel containing a mixture of iron(III) oxide, hydrogen, iron, and water at equilibrium has the following composition: compound amount Fe,O3 3.54 g H2 3.20 g Fe 4.49 g H,O 1.06 g Calculate the value of the equilibrium constant K_ for this reaction. Round your answer to 2 significant digits.

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.

The equilibrium constant, Kc, for the following reaction is 55.6 at 698 K. H2(g)+I2(g) <-----> 2HI(g) Calculate the equilibrium concentrations of reactants and product when 0.301 moles of H2 and 0.301 moles of I2 are introduced into a 1.00 L vessel at 698 K. [H2] =       M [I2]   =     M [HI] =        M

1. The diagrams below represent the following reversible chemical reaction: H2(g) + 12 (g) =2 HI (g) At 448 °C, the equilibrium constant, K, for this reaction is 51 Initial Conditions: Temperature = 448 °C Volume of the container = 2.0 L 0 = 1 mole H2 (g) = 1 mole I2 (g) 00 00 .. 00 00 •. What is the initial molar concentration of hydrogen. [H:]? What is the initial molar concentration of iodide, [I2]? M This system will reach equilibrium when rate of the forward reaction is equal to the rate of the reverse reaction. Write the equilibrium constant expression, Kc, for this reaction: Calculate the equilibrium concentrations for H;(g), I (g) and HI (g) H2(g}_ + l2 (g) 2 HI (g) [H2] [L2] [HI Initial Change Equilibrium +2x -X-

For the reaction H2(g) + Br2(g) =2 HBr(g), Kc = 81.4 at 385°C. If [H2] = [Br2] = [HBr] = 2.4 x 10-4 M at 385°C, which one of the following is correct? %3D [HBr] increases as the system approaches equilibrium. [H2] and [HBr] decreases as the system moves toward equilibrium. [H2] and [Br2] increases as the system approaches equilibrium. There is not enough information given to make a determination. [HBr] and [Br2] increases as the system approaches equilibrium. The system is at equilibrium.

Equilibrium constant, Kc, for the following reaction is 8.08×10-3 at 1080 K.2SO3(g) 2SO2(g) + O2(g)Calculate the concentration of SO3 in the equilibrium mixture?When a sufficiently large sample of SO3(g) is introduced into an evacuated vessel at 1080 K, the equilibrium concentration of O2(g) is found to be 9.70×10-2 M.

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)

For the reaction 2 NO(g) + Cl2 (g) *double arrow here* 2 NOCl (g) at 25 ℃, the equilibrium constant is 10.0. If at equilibrium, [NOCl] = 2.6 M, [NO] = 0.34 M, what is the concentration of chlorine gas?