Nitrogen reacts with hydrogen to produce ammonia according to the following equation: N2(g)+3H2(g)→2NH3(g); ΔH=-92 kJ mol-1 The energy change for this reaction is best described as
A)exothermic, because the energy of the bonds in the products is greater than the energy of the bonds in the reactants
B)endothermic, because the energy of the bonds in the products is greater than the energy of the bonds in the reactants
C)exothermic, because the energy of the bonds in the products is less than the energy of the bonds in the reactants
D)endothermic, because the energy of the bonds in the products is less than the energy of the bonds in the reactants
(I am thinking that C is correct but I am not too sure)
I'm thinking you are thinking right.
Your thinking is correct. The energy change for a chemical reaction can be categorized as either exothermic or endothermic based on the relative energies of the bonds in the reactants and products.
In an exothermic reaction, the energy released when the bonds in the products form is greater than the energy required to break the bonds in the reactants. This results in a net release of energy, usually in the form of heat. In this case, the energy of the bonds in the products is less than the energy of the bonds in the reactants.
On the other hand, in an endothermic reaction, the energy required to break the bonds in the reactants is greater than the energy released when the bonds in the products form. This means that the reaction absorbs energy from its surroundings, usually in the form of heat. In this case, the energy of the bonds in the products is greater than the energy of the bonds in the reactants.
Based on the given information, the reaction between nitrogen and hydrogen to produce ammonia has an energy change of -92 kJ mol-1. Since this energy change is negative, it indicates that the reaction is exothermic. Therefore, the correct answer is C) exothermic, because the energy of the bonds in the products is less than the energy of the bonds in the reactants.
To determine whether the reaction is exothermic or endothermic, we need to analyze the energy of the bonds in the reactants and products.
In the given equation, N2 and 3H2 are the reactants, and 2NH3 is the product. To break the bonds in the reactants, energy is required (endothermic process), while energy is released when forming the bonds in the products (exothermic process).
To determine whether the energy change is exothermic or endothermic, we compare the overall energy of the bonds in the reactants with the overall energy of the bonds in the products.
In this case, since the energy change (ΔH) for the reaction is given as -92 kJ mol-1 (negative value), it means that the reaction releases energy.
Therefore, the correct answer is A) exothermic because the energy of the bonds in the products (2NH3) is greater than the energy of the bonds in the reactants (N2 and 3H2).