For a chemical reaction that has reached dynamic equilibrium at a certain temperature, which condition is incorrect? Choose from the choices below:       continuous formation of the product       equal rate of the forward and reverse reaction       concentration of the reactant is constant       reaction comes to a halt

Why can an equilibrium be represented mathematically? Discuss the role collisions play in equilibrium reactions.

Why does this statement need to be true for chemical equilibrium to be met? The process is reversible and is in constant flux at a microscopic level. This means that the forward and reverse reactions are occurring all the time.

The elementary reaction 2H20(g)2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H20 , H2 , and O2 reach 0.053 atm, 0.0077 atm , and 0.0049 atm , respectively, at equilibrium. What is the value of the equilibrium constant at this temperature? Do not write your answer in scientific notation, give your answer as a decimal.

A system at a state of chemical equilibrium is none of these microscopically static and macroscopically dynamic. microscopically static and macroscopically static. microscopically dynamic and macroscopically dynamic. microscopically dynamic and macroscopically static.

What is meant by dynamic equilibrium? Include comparison of the rates of forward and reverse reaction

31. Please see attached image

The initial pressures of reactants and products are given for the reaction below. The reaction quotient is This means the reaction mus to reach equilibrium. shift left shift right not change 2S03 (g) = 2S02 (g) + O2 (g) K, = 16.5 atm; SO2 = 2.00 atm, 02 = 2.00 atm, SO3 = 1.00 atm

Decide whether each of the following statements is true or false.  If false, change the wording of the statement to make it true.   a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction.  d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.

When a system is a dynamic equilibrium, A no reactions are occurring B a reaction is occurring in only one direction C the rates of the forward and reverse reactions are equal D all of the reactants have been converted to products