At a certain temperature, the given reaction has an equilibrium constant of K₂ = 389. PCI, (g) + Cl₂(g) PCI, (g) PCI, is placed in a sealed container at an initial pressure of 0.0680 bar. What is the total pressure at equilibrium? P = bar

A mixture of 0.01076 mol of Cl₂, 0.04718 mol of H₂0, 0.02718 mol of HCI, and 0.01676 mol of O₂ is placed in a 1.0-L steel pressure vessel at 1846 K. The following equilibrium is established: 2 Cl₂(g) + 2 H₂O(g) = 4 HCl(g) + 1 O₂(g) At equilibrium 0.001782 mol of Cl₂ is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl₂, H₂O, HCl, and 0₂. Peq(Cl₂)= Peq(H₂O) = Peq (HCI) Peq(O₂) = = (b) Calculate Kp for this reaction. Kp =

The equilibrium constant, K. for the following reaction is 77.5 at 600 K. Co(g) + C,(g)=cOC»(g) Calculate the equilibrium concentrations of reactant and products when 0.231 moles of CO and 0.231 moles of Cl, are introduced into a 1.00 L vessel at 600K. [CO] M [CL] M [COCL] =| M

A mixture of 0.06529 mol of CH4, 0.04045 mol of H2S, 0.06585 mol of CS2, and 0.03325 mol of H2 is placed in a 1.0-L steel pressure vessel at 1304 K. The following equilibrium is established:   1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g)Peq   the equilibrium partial pressures of CH4, H2S, CS2, and H2. (CH4) =  7.5Peq(H2S) = 5.35Peq(CS2) = 6.42Peq(H2) =   1.5195   At equilibrium 0.01420 mol of H2 is found in the reaction mixture. Calculate KP for this reaction.KP = _____  .

Write the expression for the equilibrium constant K, for the following reaction. Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3 ) as (P NH3)². If either the numerator or denominator is 1, please enter 1 2 SnO2(s) 2 SnO(s) + O2(g) K =

Consider the following reaction: CO(g) + H₂O(g) = CO₂(g) + H₂(g). Exactly 200 torr each of CO and water vapor were introduced into a 500 ml flask. When the mixture reached equilibrium at 800 K, the partial pressure of CO2 was found to be 99 torr. Calculate the value of Kp.

A sample of N₂H6CO₂ weighing 22.5 grams is heated to 80°C in a 1.0 L container. All of the salt sublimes into NH3(g) and CO₂(g) according to the following equilibrium process. N₂H6CO₂ (s) + CO₂ (g) + 2NH3 (g) Determine the partial pressure of the NH3(g) in the system in atmospheres. This discussion is closed. M CAL -:00- 0:50- CI 2:00 Submit Answer Tries 0/99 3 F1 @ 2 ост 21 9: F2 3 80 F3 $ 4 10 a F4 % 5 S F5 6 tv A MacBook Air C F6 & 7 F7 ( Î DII FB F9 F10 F11 54 F13 Send 22

A sample of NH4HS(s) is placed into a 1.60 L vessel containing 0.170 g NH3. What is the total gas pressure when the system reaches equilibrium at 298.15 K? The reaction is: NH4HS(s) = NH3(g) + H2S(g) Kp = 0.108

Bromine monochloride is synthesized using the reaction Br₂(g) + Cl₂(g) 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 191.0 L flask initially contains 1.055 kg of Br₂ and 1.124 kg of Cl₂. Calculate the mass of BrCl, 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: 50 g %

A chemical engineer is studying the following reaction: HCH3CO2(aq)+CH3NH2(aq) → CH3CO2(aq)+CH3NH(aq) At the temperature the engineer picks, the equilibrium constant K for this reaction is 0.80. The engineer charges ("fills") four reaction vessels with acetic acid and methylamine, and lets the reaction begin. She then measures the composition of the mixture inside each vessel from time to time. Her first set of measurements are shown in the table below. Predict the changes in the compositions the engineer should expect next time she measures the compositions. reaction vessel compound concentration expected change in concentration HCH CO₂ 0.58 M ↑ increase ↓ decrease (no change) CH3NH2 0.57 M ↑ increase ↓ decrease (no change) A CH3CO2 1.09 M ○ ↑ increase ↓ decrease (no change) CH,NH, 1.28 M ○ ↑ increase ↓ decrease (no change) HCH,CO₂ CH3NH2 1.28 M ↑ increase ↓decrease (no change) 1.27 M ↑ increase ↓ decrease (no change) B CH,CO, 0.39 M ↑ increase ↓ decrease (no change) CHÍNH, HCH3CO2…