True: At dynamic equilibrium, the forward and backward reactions happen at the same time, An exothermic reaction releases thermal reactions to the surroundings, A closed system is one in which no chemicals can enter or leave, This is the sign for a reversible reaction, At equilibrium the forward and backward reaction happen at the same rate, At equilibrium, the concentration of the reaction mixture stays the same, If the forward reaction is exothermic then the reverse is endothermic, The forward reaction is endothermic 2A + B ⇌ C + D. An increase in temperature will cause equilibrium to shift right , 2A + B ⇌ C + D. An increase in pressure will increase the yield of C+D, False: The forward reaction is the reaction to the left, Endothermic reactions have a negative energy change, An open system is needed to reach dynamic equilibrium, This sign is for a reversible reaction, At equilibrium, no reaction happens, The reaction mixture always has 50% reactants and 50% products, This is a reaction profile for an endothermic reaction, 2A + B ⇌ C + D. Removing A and B will increase the yield of C and D, 2A + B ⇌ C + D There is more A and B than C and D,

Dynamic equilibrium

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