Consider the reaction 2 H 2 + O 2 ⟶ 2 H 2 O Δ H rxn = − 484 kJ Which answer best describes the transfer of heat that occurs when 1.60 mol H 2 reacts? 387 kJ absorbed 484 kJ released 387 kJ released 774 kJ absorbed 484 kJ absorbed 774 kJ released

387 kJ energy is released

Explanation:

Endothermic reactions: These are the reactions in which energy is required in the reaction. The energy of the products are more than the energy of the reactants. is positive.

Exothermic reactions: These are the reactions in which energy is released in the reaction. The energy of the products is less than the energy of the reactants. is negative.

The given balanced equation is ;

According to stoichioetry :

2 moles of hydrogen reacts to give = 484 kJ of heat

Thus 1.60 moles of hydrogen reacts to give =

Thus 387 kJ energy is released

a

each chemical family is represented as a group or column on the periodic table. based on chemical properties, there are 6 types of chemical families. group 1 represents alkali metals, group 2 represents alkaline earth metals, groups 3 to 12 represent transition metals, groups 13 to 16 represent non-metals and other metals, group 17 represents halogens and group 18 represents noble gases.