Question

CHEM 1110-01 Lecture Questions Monday February 26, 2018 1. The equilibrium constant K. for the following reaction is 5.10 × 10. at 548K: Calculate the equilibrium concentrations of HCI when 0.270 moles of NH,Cl L vessel at 548 K are introduced into a 1.00 2. The equilibrium constant K, for the following reaction is 10.5 at 350 K Calculate the equilibrium partial pressures of all species when CH Cl2 flask at a pressure of 0.775 atm at 350 L is introduced into an evacuated 3. Hig, and '2 ia, were added to a heated container. [Hal。= 0.0 100 mol At equilibrium [12]eq-0.00500 mol L-1. Determine Kc given and 111,-0.00800 mol . 4. Suppose a 500 mL flask is filled with 1.2 moles of O2 and 1.4 moles of NO. The following reaction becomes possible The equilibrium constant Ke for this reaction is 0.300 at the temperature of the flask. Calculate the equilibrium molarity of N2

Please be detailed in solving one step by step

(Any one question)

Answer 1

3 Ce In ha -싯 t2以 ehama 2ス 2(o.os 2-ano or)m О. о о 3 m 3 6 x 3 5 X it Ke = 1.0286~ 1.03