Question

Is the change in enthalpy for a reaction an extensive property? Explain the relationship between \(\Delta H\) for a reaction and the amounts of reactants and products that undergo reaction.

Short answer

\(\Delta H\) is an extensive property because it depends on the scale of the reaction.

Step-by-step solution

Define extensive property

Identify and explain an extensive property. An extensive property of a system depends on the system size or the amount of matter in the system. Examples include mass, volume, and enthalpy.

Explain the relationship between \(\Delta H\) and the reaction scale

Explain that the change in enthalpy (\(\Delta H\)) for a reaction is directly proportional to the amounts of reactants and products involved in the reaction. If the scale of the reaction is doubled, so is the \(\Delta H\).

Determine if \(\Delta H\) is an extensive property

Given that \(\Delta H\) changes with the amount of reactants and products, it is an extensive property because it scales with the system size.

Key concepts

Extensive Property

When you hear scientists talk about extensive properties, what they mean are characteristics that change when the size of the sample changes. Think of it like making a recipe – if you double the ingredients, you’ll get double the cake! Much like your cake, an extensive property grows with the amount. Some familiar examples of extensive properties are the mass and volume. If you take twice as much of a substance, its mass and volume will double. This is important in chemistry because it helps us understand how a substance behaves when we have more or less of it.

Enthalpy, which we represent as \( \Delta H \), is also an extensive property. This means if we were to scale up a chemical reaction, say perform it with twice as many reactants, the total enthalpy change or 'heat content' involved in the process would also double. This is a crucial concept when considering how much energy is required for industrial-scale reactions compared to small laboratory experiments.

Enthalpy (\(\Delta H\))

Enthalpy change, conveniently symbolized as \(\Delta H\), is a bit like the energy currency of chemical reactions. It's a measure of how much heat is absorbed or released during a chemical reaction at constant pressure. When the products of a chemical reaction have lower energy than the reactants, \(\Delta H\) is negative, and we say the reaction is exothermic – it gives off heat. On the flip side, if the reaction requires energy input because the products are higher in energy, \(\Delta H\) is positive, and the reaction is endothermic.

We express this value on a per-mole basis, meaning it's given for a certain quantity of reactant, but remember, since it's an extensive property, the actual amount of heat involved will change in proportion to the amount of reactant we start with. This leads to interesting calculations for how much energy is needed or released when scaling reactions up or down.

Stoichiometry

Stoichiometry can be a bit daunting, but it's essentially the math behind chemistry. It's about figuring out exactly how much of each substance is involved in a chemical reaction. It relies on the principle of conservation of mass; atoms are neither created nor destroyed in a chemical reaction. So, if you know the amounts of your reactants, you can predict the amounts of products you’ll get.

Through stoichiometry, we link the balance of equations (the recipe of our reaction) with the enthalpy change. By doing this, we can calculate exactly how much energy will be used or produced when we mix certain amounts of reactants together. Imagine baking without a recipe – your cake could end up a mess! Stoichiometry gives us the 'recipe' for making sure our reactions go to plan.

Chemical Reactions

Chemical reactions are the heart of chemistry. They're about substances changing into new substances – transforming reactants into products. This transformation happens because atoms rearrange themselves in new ways. For instance, when you light up a grill, the charcoal (carbon) reacts with oxygen in the air to create carbon dioxide. That's a chemical reaction.Not all reactions are made equal. Some occur spontaneously, while others need a bit of encouragement, like heat, light, or electricity. And as these reactions happen, they observe the laws of stoichiometry: atoms are conserved, and the enthalpy change tells us how much energy comes in or out. Grasping the basics of chemical reactions allows us to predict how substances will interact, understand product formation, and control the conditions to get the best yield – whether that be in a lab test tube or industrial vat.