2Na(s) + 2H2O(aq) = 2NaOH (aq) + H2 (g)
Is this reaction exothermic or endothermic? I don't understand ,
If you've ever dropped sodium into water, you know that the reaction is violently exothermic.
What is conservation of mass
To determine if a reaction is exothermic or endothermic, we need to analyze the energy changes that occur during the reaction.
In an exothermic reaction, energy is released into the surroundings, usually in the form of heat. This means that the products have lower energy than the reactants.
In an endothermic reaction, energy is absorbed from the surroundings, usually in the form of heat. This means that the products have higher energy than the reactants.
Looking at the given equation:
2Na(s) + 2H2O(aq) = 2NaOH (aq) + H2 (g)
We can see that sodium (Na) and water (H2O) react to form sodium hydroxide (NaOH) and hydrogen gas (H2). The formation of hydrogen gas indicates a release of energy, which suggests an exothermic reaction.
Therefore, the given reaction is exothermic.
To determine whether a reaction is exothermic or endothermic, you need to consider the overall energy change that occurs during the reaction. In this case, you can analyze the reaction by looking at the energy released or absorbed when bonds are broken or formed.
The reaction you provided is the reaction between sodium (Na) and water (H2O) to form sodium hydroxide (NaOH) and hydrogen gas (H2). Let's break down the reaction into individual bond breaking and bond formation steps:
1. Breaking bonds: In the reactants (2Na + 2H2O), you need to break the bonds between sodium and chlorine (Na-Na) and between hydrogen and oxygen (H-O-H). Breaking these bonds requires energy input, as energy needs to be supplied to overcome the attractive forces between the atoms.
2. Forming bonds: In the products (2NaOH + H2), new bonds are formed between sodium and hydroxide (Na-OH) and between the two hydrogen atoms (H-H). Formation of bonds releases energy because atoms are now in a more stable configuration with lower potential energy.
To determine if the reaction is exothermic or endothermic, you need to compare the energy required to break the bonds (endothermic process) with the energy released when new bonds are formed (exothermic process). If the energy released is greater than the energy required, the reaction is exothermic (more energy is released than absorbed). Conversely, if the energy required is greater than the energy released, the reaction is endothermic (more energy is absorbed than released).
In this case, breaking the bonds in the reactants requires energy, but the formation of new bonds in the products releases more energy. Therefore, the overall energy change during this reaction is exothermic.