Is the enthalpy for this reaction positive or negative?

Enthalpy is the amount of heat content used or released in a system

By looking at whether q is exothermic or endothermic we can determine a relationship between \(\Delta H\) and \(q\). If the reaction absorbs heat it is endothermic meaning the reaction consumes heat from the surroundings so \(q > 0\) (positive). If q is positive then \(\Delta H\) is also positive. And the same goes for if the reaction releases heat, then it is exothermic, meaning the system gives off heat to its surroundings, so \(q < 0\) (negative). If \(q\) is negative, then \(\Delta H\) will also be negative.

So if your Delta H is positive it requires energy to proceed

yes you are right

+ve enthalpy = endothermic = absorbs heat from surroundings

- ve enthalpy = exothermic = released heat into the surroundings.

enthalpy is a measure of the stored potential energy within the bonds of the species involved. Therefore if the enthalpy is +ve, more energy is required to break old bonds, than is released when new bonds are formed..ie, energy is required from the surroundings in order for the reaction to take place (reactions achieve activation energy)