Question

A reaction has a value of ΔH = -30 kJ/mol. What do you know about the reaction? The reaction is not at equilibrium

The products predominate once it reaches equilibrium
The reaction will have a very slow rate
When it reaches eq, very little product will be present
We cannot conclude anything about equilibrium from this data

Answer 1

Answer: The products will predominate once it reaches equilibrium

Step-by-step explanation:

ΔH refers to the change in enthalpy in a system. It allows to to understand whether heat was absorbed or given away during a process.

Usually when ΔH > 0, the reaction in endothermic, meaning heat was absorbed. When heat is absorbed, equilibrium shifts towards the right side of the chemical equation, where the reactants are written.

When ΔH < 0, like this problem where ΔH = -30 kj, the reaction is exothermic and heat is given off during the process. In order to balance the reaction, equilibrium will shift to the left, towards the products.