At 21.8°C, Keq = 7.0  10-2 for the equilibrium shown below. NH4HS(s)  NH3(g) + H2S(g) Calculate the equilibrium partial pressures of NH3 and H2S if a sample of solid NH4HS is placed in a closed vessel and decomposes until equilibrium is reached. NH3  ______ atm H2S  ______ atm

Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5⁢(g)⁢↽−−⇀⁢PCl3⁢(g)+Cl2⁢(g) A 13.1 gsample of PCl5 is added to a sealed 1.25 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 48.4% of the PCl5 remains. What is the equilibrium constant, Kc , for the reaction?

The following reaction is at equilibrium: N2{g) + 3H2(g)22NH3(g) The equilibrium concentration for N2 and H2 are 0.22 M and 0.4 M, respectively. If the Keq is 0.78, what is the equilibrium concentration of NH3? Enter your answer using 3 decimal places and without unit.

Consider the following equilibrium system: 2 NOCI(g) 2 2 NO(g) + Cl2(g) Kc = 57.0 Initially, only NOCI gas is placed in a flask. After equilibrium has been reached it is found that the concentration of the nitrogen monoxide gas in the flask is 1.14 mol/L. What is the initial molar concentration of the NOCI gas? Answer to three decimal places.

Answers are attached. Please show all steps and make an ICE table. Thank you!

Which answer below correctly describes the calculation to find the equilibrium expression for K4? Co(g) + 3H2(g) CS2(g) + 2H2S(g) CH4(g) + H20(g) K1 CH4(g) + 2S2(g) K2 CO(g) + H20(g) CS2(g) + 2H2S(g) + 3CO2(g) = 4CO(g) + 2S2(g) + 2H20(g) CO2(g) + H2(g) K3 K4 Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. K1 x (K2)¬1 x (K3)³ a b K1 x K2 x K3 3(K) x K х Кз d K1 x K2 x (K3)³ Use the following series of reactions to determine the value of the equilibrium constant K.j: NOz + H30+ - C5H5NH+ + OH- 2H20(1) = H30+ + OH° C5H5N + HNO, = C5H5NH+ + NO, Reaction1: HNO2 + H20(1) Kcı =?? -6- Reaction2 : C5 H5N + H20(1) Kc2 = 1.70 × 10 Reaction3 : Ксз — 1.01 X 10 14 Reaction4 : Kc4 = 1.19 x %3D Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 7.07 X 10-4 b 2.01 X 10-25 9.93 X 1024 d 4.17 X 10-24 6.86 X 1034 e

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Iron and water react to form iron(III) oxide and hydrogen, like this: 2 Fe(s) + 3 H₂O(g) → Fe₂O3(s)+ 3 H₂(g) At a certain temperature, a chemist finds that a 2.5 L reaction vessel containing a mixture of iron, water, iron(III) oxide, and hydrogen at equilibrium has the following composition: compound Fe H₂O Fe₂O3 H₂ amount 4.04 g 2.87 g 3.49 g 2.08 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. C K = 0 C Dx1 x10 X Ś

▸ 69 20 E Consider the following system at equilibrium at 723 K: N₂(g) + 3H₂(g) 2NH3(g) + 26.6 kcal Indicate whether each individual change would favor the production of NH3(g). Evaluate each change separately, assuming that all other conditions remain constant. D Decreasing the temperature. Decreasing the pressure. Increasing the volume. Removing NH3. Removing H₂. C Submit Answer $ 4 R F % 5 V Retry Entire ♫ FS T G [References] the References to access important values if needed for this question. A 6 v yes no B MacBook Air F6 3 more group attempts remaining Y H & 7 B F7 U N * 8 00 D--ll FB J J ( T 1 M 9 K DD FO O O L ge A F10 P command Previous Email Instructor 4 i A AN = Next> Save and Exit ( { ? 912 option delete retu