equilibrium concentration

General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science presented by Macmillan Phosphorus pentachloride decomposes according to the chemical equation PCI, (g) = PCI, (g) + Cl, (g) K. = 1.80 at 250 °C A 0.2584 mol sample of PCI, (g) is injected into an empty 3.65 L reaction vessel held at 250 °C. Calculate the concentrations of PCl, (g) and PCl, (g) at equilibrium. [PCI5] = || 0.005 Incorrect [PCI,] = 0.066 Incorrect

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Suppose a 250. mL flask is filled with 0.10 mol of CO, 0.30 mol of H,O and 1.8 mol of H,. The following reaction becomes possible: co(g) + H,0(g) =CO,{g)+H2(g) The equilibrium constant K for this reaction is 0.296 at the temperature of the flask. Calculate the equilibrium molarity of H,0. Round your answer to two decimal places.

Suppose a 250. mL flask is filled with 0.10 mol of N, and 1.8 mol of NO. The following reaction becomes possible: N2(g) + 0,(g) == 2NO (g) The equilibrium constant K for this reaction is 0.422 at the temperature of the flask. Calculate the equilibrium molarity of O2. Round your answer to two decimal places. IM ?

Suppose that 8.00 mol of both O2 and N₂O gases are introduced into a 4.00 L closed flask. When the system comes to equilibrium, 3.00 mol of nitrogen monoxide (NO) gas has formed, shown below. Determine the equilibrium concentrations of all entities in the flask. 2 N₂O(g) + O₂ (g) = = 4 NO(g) UPLOAD A FULL SOLUTION WITH AN ICE TABLE, CALCULATIONS, AND FINAL ANSWERS WITH UNITS AND THE CORRECT NUMBER OF SIGNIFCANT DIGITS.

Be sure to answer all parts. The equilibrium constant Kc for the reaction 2NH3(g) = N2(g) + 3H2(g) is 0.83 at 375°C. A 23.7 g sample of ammonia is placed in a 6.00 L flask and heated to 375°C. Calculate the concentrations of each gas when equilibrium is reached. [NH3leq M [N2leg = M [H2leq M

1 atm = 760 mm Hg R = 0.0821 L atm/ mol K K = °C + 273 PV = nRT Molar volume @ STP, 1 mole = 22.4L of ideal gas 1. produce nitrogen gas. One important reaction is listed below The inflation of an automobile airbag involves several chemical reactions that 10NA(s) + 2KNO3(s) –> K2O(s) + 5Na2O(s) + N2(g) If a side airbag contains 71.3 g Na and 75.9 g KNO3, to what pressure, in mm Hg, would a 5.30 L airbag inflate (due to the production of nitrogen gas) if the reaction occurs at a temperature of 72.0°C.

6 of 12 Part A I Review | Constants Periodic Table Determine the value of the equilibrium constant, Kgoal, for the reaction CO2(g) = C(s) + O2(g), Kgoal =? by making use of the following information: 1. 2CO2(g) + 2H2O(1) = CH;COOH(1) + 202(g), K = 5.40 x 10-16 2. 2H2 (g) + O2(g) = 2H,0(1), K2 1.06 x 1010 3. CH3COOH(1) = 2C(s) + 2H2(g) + O2(g), K3 = 2.68 x 10-9 Express your answer numerically. • View Available Hint(s) 中。 goal = 5:08 AM 19 3/1/2021

Given the reaction between two gases represented by A2 and B2 to give the compound AB(g) A2(g) + B2 +B2(g) 2AB(g) At equilibrium, the concentration of A₂ = 3.0 × 10³M, of B₂ = 4.2×103 M, of AB = 2.8×103 M. If reaction takes place in a sealed vessel at 527°C, then the value of K, will be Options: (a) 2.0 (b) 1.9 (c) 0.62 (d) 4.5