If AG° < 0, then at equilibrium there will be more products than reactants. false true

1.5 mol of PCI5 was placed in a 1.0 L container and allowed to reach equilibrium. At equilibrium, the [PCI5] was found to be 1.2 mol/L. What is the Keq value for the reaction below? Your solution must include an ICE chart. Please factor in significant figures into your response. PC|3(g) + Cl2(g) PC15(g) The equilibrium system shown below has a Keq = 1.4 x 10-4. If [A] = 0.24 mol/L, what is the [D]? Please factor significant figures into your answer. Please write your answer in the following format 3A(g) + B(s) C(s) + 2D (g)

Questions from Lab: Equilibrium and Le Chatelier's Principle 1.Consider the chemical reaction: N2+ 3H2 yields 2NH3. The equilibrium constant is K = 6.0 x 10-2, and concentrations are as follows [H2] = 2.5 x 10-1 M, [N2] = 4.0 M, and [NH3] = 1.0 x 10-4 M. Is the reaction at equilibrium? If not, which direction would it shift? Show your calculations.   2. Given this reaction at equilibrium, C(s) + CO2(g) D 2CO(g) (∆H° = 119kJ), explain the changes that would occur when the following stresses are applied: a.CO is removed. b.Heat is removed. c.CO2 is added.

How will an increase in temperature affect the following equilibrium? How will a decrease in the pressure of the reaction vessel affect it? 302 (g) 203 (g) AH = 285 kJ An increase in temperature will shift the equilibrium to the left; a decrease in the pressure of the reaction vessel will shift the equilibrium to the right O An increase in temperature will shift the equilibrium to the right; a decrease in the pressure of the reaction vessel will shift the equilibrium to the right O An increase in temperature will shift the equilibrium to the right; a decrease in the pressure of the reaction vessel will shift the equilibrium to the left. An increase in temperature will shift the equilibrium to the left; a decrease in the pressure of the reaction vessel will not affect the equilibrium

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When solving equilibrium problems with a very large Keq, the best way to simplify the problem is to approach equilibrium from the product side of the reaction. True False

CO(g) + H2O(g) ↔️ CO2(g) + H2(g)     (Keq = 0.58) If 1.00 mol each of carbon monoxide and water are placed in a 50.0L rigid container, what will the equilibrium concentration of hydrogen gas be?

Need help understand question 2 a,b,c

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Consider the following reaction at equilibrium in the gas phase: N2O4   double arrows    2 NO2 Which direction will the equilibrium shift when more nitrogen dioxide is added?     To the left     To the right     Neither