The student collects the H2(g) produced by the reaction and measures its volume over water at 298 K after carefully equalizing the water levels inside and outside the gas-collection tube, as shown in the diagram below. The volume is measured to be 45.6mL . The atmospheric pressure in the lab is measured as 765 torr , and the equilibrium vapor pressure of water at 298 K is 24 torr. 1. Find the number of moles of H2 (g) produced in the reaction

Bromine monochloride is synthesized using the reaction Br, (g) + Cl, (g) = 2 BrC(g) K, = 1.1 x 104 at 150 K A 201.0 L flask initially contains 0.951 kg of Br, and 1.116 kg of Cl,. Calculate the mass of BrCI, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCl: What is the percent yield of BrCl? percent yield:

N204(g) = 2 NO2(g) Three experiments were run starting with different initial amounts of N2O4(g) ([N204]o in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO2 and N204 at equilibrium. Be sure to round to the correct number of significant figures. Exp[N204l0 [NO2][N,04] [NO,] / [N204] 2 [NO,] / [N204] [NO2]? / [N204] 1 3.7 2.92 2.2 2 3.0 2.56 1.7 3 2.3 2.15 1.2 Based on your calculations, indicate whether each statement is True (T) or False (F): v1. Each experiment started with a different initial concentration of N204. v2. The ratio ([NO2] / [N204]) is equal to a constant value. v3. The ratio (2 [NO2] / [N204]) is equal to a constant value. v 4. The ratio ([NO2]? / [N204]) is equal to a constant value. v5. Each experiment reached a…

2 CO(g) + O2(g) +2 CO2(g) K = 6.1 x 105 If [CO] = 0.00100 M and [O2] = 0.00127 M, determine [CO2], in M.