Consider the following system at equilibrium where AH = -87.9 kJ, and Kc = K: PC13 (g) + Cl₂ (g) ⇒ PC15 (9) If the temperature on the equilibrium system is suddenly decreased: The value of Ke O increases O decreases O remains the same The value of Q O is less than Ke O is greater than O is equal to Kc The reaction must Orun in the forward direction to reestablish equilibrium O run in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of Cl₂ will O increase O decrease O remain the same 83.3, at 5.00 × 10²

The equilibrium system shown below was analyzed and the concentrations of H2(g), I2(g) and HI(g), were found, in mol/L, to be 4.2, 3.8, 1.6 respectively. The equilibrium constant must be? H2(g) + I2(g) <=====> 2HI(g) + 65 kJ

Consider the following reaction at equilibrium. What effect will doubling the temperature have on the system? CH4 ( + 2 02 () = CO2 (g) + 2 H2O () AH° = -882.0 kJ O No shift will occur because the volume of the system has not changed. No shift will occur because the total number of gas molecules on both sides of the chemical equation are equal. O A shift left towards reactants will occur. O No shift will occur because none of the concentrations have changed. O A shift right towards products will occur.

Use the following information to answer the next question Factors that can affect equilibrium I and II III only I, II, and III I. O II only II. III. The factors from the list above that would increase the equilibrium concentration of NO(g) in the system; 4NH3(g) +502 (g) 4NO(g) + 6H₂O(g) AH = -905 kJ while all other variables are held constant are Decreasing the volume Increasing the temperature Adding NH3(g)

Why would answer choice (c) for question 16 be correct?

Please answer ALL parts of the question and show your work. Consider this reaction: 2H2S(g) + 3O2(g)  <-----> 2H2O(g) + 2SO2(g)       H= -1036 kJ Predict whether the forward or reverse reaction will reestablish equilibrium is disturbed by (a) expanding the container (b) removing SO2 (c) rasing the temperature (d) water vapor is added

For the equilibrium system below, which of the following would result in an increase in the quantity of H₂(g)? H₂(g) + 12(g) 2HI(g) + 65 kJ ос removing some I₂(g) and removing some HI(g) removing some HI(g) removing some 1₂(g) decreasing temperature removing some HI(g) and decreasing temperature

Consider the following system: 4 NH3(g) + 3 O2(g) -> 2 N2(g) + 6 H2O(l) AH = -1530.4 kJ (a) How will the amount of ammonia at equilibrium be affected by      (1) removing O2(g)?      (2) adding N,(g)?      (3) adding water?      (4) expanding the container at constant pressure?      (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?