Bromine monochloride is synthesized using the reaction Br, (g) + Cl, (g) 2 BrCl(g) K, = = 1.1 x 10-4 at 150 K A 199.0 L flask initially contains 1.096 kg of Br, and 1.195 kg of C,. Calculate the mass of BrCl, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: Enter numeric value What is the percent yield of BrCl? percent yield: %

The equilibrium constant, K., for the following reaction is 1.29×102 at 600 K. COCI,(e)=CO(g) + Cl,(g) Calculate the equilibrium concentrations of reactant and products when 0.270 moles of COCl2(g) are introduced into a 1.00 L vessel at 600 K. [COC,] = | M [CO] M [Cl,] M

At a certain temperature, 0.347 mol CH, and 0.619 mol H,S are placed in a 2.50 L container. CH,(g) + 2 H, S(g)= CS, (g) + 4 H,(g) At equilibrium, 11.8 g CS, is present. Calculate K.. K. =

O KINETICS AND EQUILIBRIUM 1/5 Calculating equilibrium composition from an equilibrium constant Suppose a 500. mL flask is filled with 1.1 mol of Cl,, 0.20 mol of HCl and 0.80 mol of CCl,. The following reaction becomes possible: Cl,(g) +CHCI, (g) = HCl(g)+CCl, (g) The equilibrium constant K for this reaction is 9.65 at the temperature of the flask. Calculate the equilibrium molarity of HCl. Round your answer to two decimal places. | M II

Calculating equilibrium composition from an equilibrium... 0/5 Suppose 500. mL flask is filled with 1.9 mol of H, and o0.50 mol of C1,. The following reaction becomes possible: H, (g) + Cl,(g) – 2HC1(g) The equilibrium constant K for this reaction is 3.61 at the temperature of the flask. Calculate the equilibrium molarity of H,. Round your answer to two decimal places. OM

Suppose a 500. mL flask is filled with 0.80 mol of H, and 0.90 mol of HI. The following reaction becomes possible: H, (g) +1,(g) – 2HI(g) The equilibrium constant K for this reaction is 3.50 at the temperature of the flask. Calculate the equilibrium molarity of I,. Round your answer to two decimal places. ?

please provide detailed solution and give the explanation of the concept....     A student ran the following reaction in the laboratory at 656 K: 2NH3(g) N2(g) + 3H2(g) When she introduced 8.62×10-2 moles of NH3(g) into a 1.00 liter container, she found the equilibrium concentration of H2(g) to be 0.118 M. Calculate the equilibrium constant, Kc, she obtained for this reaction. Kc = ?

Suppose a 500. mL flask is filled with 0.20 mol of Cl, and 1.5 mol of HCl. The following reaction becomes possible: H,(2) + Cl, (g) – 2HCI(3) The equilibrium constant K for this reaction is 0.754 at the temperature of the flask. Calculate the equilibrium molarity of Cl,. Round your answer to two decimal places. |M ?

3. Initially 2.25 mol of carbon monoxide gas, CO) and 2.25 mol of water vapour, H₂O(g), are placed in a 1.50 L container and equilibrium is established and Keq is 4.2. Determine all equilibrium concentrations. CO (6) + H₂O (8) [02]}} + H₂

At a certain temperature, 0.3011 mol of N₂ and 1.781 mol of H₂ are placed in a 4.00 L container according to the following equation: N₂(g) + 3H2(g) + 2NH3(g) At equilibrium, 0.1401mol of N₂ is present. Calculate the equilibrium constant.