What does each symbol represent? K Gibbs free energy reaction quotient Greek lowercase mu mole fraction activity equilibrium constant G chemical potential molar concentration a

Define equilibrium constant Keq

Consider the following equilibrium reaction:H2(g) + I2(g) ↔ 2HI(g)If the following equilibrium concentrations are observed: [H2] = 4.10 x 10-1M, [I2] = 5.54 x 10-2M, [HI] = 3.50 x 10-2M; what is the equilibrium constant

If the equilibrium constant of a given reaction is 2.10, what is the equilibrium constant of its reverse reaction?

If the equilibrium constant of a given reaction is 6.69, what is the equilibrium constant of its reverse reaction?

The equilibrium system between nitrogen gas, oxygen gas, and nitrogen dioxide gas is given N2(g) + 2O2(g)----->2N2(g) Write the balanced chemical equation for the reverse reaction. Include physical states

Indicate whether or not product formation increases if the size of the reaction container is decreased for each of the following equilibrium systems. a) 4NH3(g) + 5O2(g)  heat + 4NO(g) + 6H2O(g)                                b) heat + 2NaHCO3(s)   Na2CO3(s) + CO2(g) + H2O(g)

Consider the system N2(g) + 3 Cl2(g) 2 NCI3(g) AH = +232 kJ Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by each of the following. decreasing the temperature removing nitrogen trichloride gas 1. forward reaction compressing the system at constant temperature 2. reverse reaction adding chlorine gas

Consider the following exothermic reaction system at equilibrium: N2(g) + 3H2(g) ⇒ 2NH3(g) Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below: Note: Use I for increase, D for decrease, NC for no change Add N2(g) Remove H2(g) Add NH3(9) Add Ne(g) Increase the temperature (constant P) Decrease the volume (constant T) Add a catalyst Submit NH3 N₂ H2