Consider the following reaction at equilibrium:  2NH3 (g) ↔ N2 (g) + 3H2 (g) ΔH° =46.1 kJ at 298K  Is the following remark true or false? The forward direction is favored when the equilibrium is disturbed by an increase in temperature.  (A)True (B)False

Consider the following system at equilibrium where Ho = 18.8 kJ, and Kc = 9.52E-2, at 350 K: CH4(g) + CCl4(g) 2 CH2Cl2(g) If the VOLUME of the equilibrium system is suddenly decreased at constant temperature:   whats the value of Kc   The value of Q   The reaction must

14.98 The equilibrium constant Kc for the synthesis of methanol (i.e. CH3OH) with reaction CO(g) + 2H2(g) CH3OH8) is 4.3 at 250 °C and 1.8 at 275 °C. Is this reaction endothermic or exothermic?

What is the effect of equilibrium when heat is removed (cooled) from the system? CO + H2O ⟷ CO2 + H2 ΔH = +41.4 kJ Group of answer choices Neither reactant nor products would be produced. Shift left. Both reactants and products would be produced. Shift right. This equation does not represent an equilibrium system.

Consider the following equilibrium: N2 (g)+3H2(g)2NH3 (g) AG = -34. kJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: OO rise ☐ x10 fall OO Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H2? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm S

When wine spoils, ethanol is oxidized to acetic acid as oxygen from the air dissolves in the wine. C₂H5OH (aq) + O₂ (aq) = CH3COOH (aq) + H₂O (1) The value of Keq for this reaction at 298K is 1.2 x 108²2. Will there be much ethanol remaining when the reaction has reached equilibrium? Explain.

38. For this process at 25 °C: H2O(g) H2O (A) AH is negative as energy is released. (B) AH is negative as energy is absorbed. (C) AH is positive as energy is released. (D) AH is positive as energy is absorbed.

(a)        N2(g)               +          O2(g)                           2NO (g)            ∆H298 = + 180 kJ mol-1    From the equilibrium shown above, use Le Chatelier’s Principle to decide what happens to the equilibrium position by:   Increasing the concentration of NO Increasing the pressure Increasing the temperature Increasing the concentration of N2 Adding a catalyst