[Review Topics] [References] Consider the following system at equilibrium where AH = 92.7 kJ, and Kc = 1.80 x 10-4, at 298 K. NH HS(s)→ NH3(g) + H₂S(g) When some moles of NH4HS(s) are added to the equilibrium system at constant temperature: The value of Ke Oincreases Odecreases Oremains the same The value of Qc Ois greater than Ke O is equal to Ke O is less than Ke The reaction must Orun in the forward direction to reestablish equilibrium. Orun in the reverse direction to feestablish equilibrium. Oremain the same. It is already at equilibrium. The number of moles of NH3 will Oincrease Odecrease Oremain the same Submit Answer Retry Entire Group 9 more group attempts remaining Show Hint Previous Next>

Express the equilibrium constant for the following reaction.

Q1) For the equilibrium: A B, if [A].0.569, [B].0.162, and Kea 47.8, what are [A]es and [B]ea? algebraic expression: [A]eq= Q2) For the equilibrium: 1221, if [2]. 1.26, [1].0, and Keq = 1.14 x10, what are [12]eg and [lleg? E algebraic expression: [H₂leq_ [12]eg [B]ea. algebraic expression: [12]ea. [eq M Q3) For the equilibrium: H₂ + 1₂2H1, if [H₂lo=0.546, [b]o 1.26, [HI].0, and Kea 45.3, what are [Halea, [lzles and [HI]eq? =0 [HI] eq = 0 0

Hydrogen and chlorine react to form hydrogen chloride, like this: H,(g) + Cl,(g) 2 HCl(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen, chlorine, and hydrogen chloride has the following composition: compound concentration at equilibrium 0.86 M Cl, 0.30 M HC1 1.9 M Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. K = 0