Chapter 2: Problem 126
Write the balanced gas phase chemical equation for the reaction of dinitrogen pentoxide with sulfur dioxide to form sulfur trioxide and nitrogen oxide. What small, whole-number ratios are expected for oxygen in the nitrogen oxides and the sulfur oxides?
Short Answer
Expert verified
The balanced equation is (NO2)5 + SO2 -> 2SO3 + 2NO2. The whole-number ratios for oxygen are 2:1 for NO2 and SO2, and 3:1 for SO3.
Step by step solution
01
Write the Unbalanced Equation
Write the chemical formulae of the reactants and products. The reactants are dinitrogen pentoxide ((NO2)5) and sulfur dioxide (SO2), and the products are sulfur trioxide (SO3) and nitrogen oxide (NOx, where x is to be determined). The unbalanced equation is: (NO2)5 + SO2 -> SO3 + NOx.
02
Determine the Products
Determine the correct formula for nitrogen oxide. Since the oxygen atoms must be balanced and we have three types of oxides, observing the trends in oxidation states can help us determine that the likely product for nitrogen oxide is NO2. This is because NO and NO2 are the most common nitrogen oxides. By comparing oxygen count, NO2 makes sense for balancing. Now the tentative unbalanced equation is: (NO2)5 + SO2 -> SO3 + NO2.
03
Balance the Atoms Other Than Oxygen
Begin by balancing the number of N and S atoms on both sides. There are 2 N atoms on the left side, so we must have 2 N atoms on the right. Balance S by ensuring there is 1 S atom on both sides. Now look at the Nitrogen, which gives us two molecules of NO2 for every (NO2)5 molecule. The temporary unbalanced equation becomes: (NO2)5 + SO2 -> SO3 + 2NO2.
04
Balance the Oxygen Atoms
Finally, balance the number of O atoms. There are 10 O atoms from (NO2)5, and 2 from SO2, giving a total of 12 O atoms on the reactant side. On the product side, there are 3 O atoms in SO3 and 4 O atoms from 2NO2 (2 NO2 molecules), giving a total of 7 O atoms. To balance the O atoms, add another SO3 molecule to the product side. The final balanced equation is: (NO2)5 + SO2 -> 2SO3 + 2NO2.
05
Determine Whole-Number Ratios for Oxygen
Examine the oxygen content in the nitrogen and sulfur oxides. Nitrogen oxide here is NO2, which has a 2:1 oxygen-to-nitrogen ratio. For sulfur oxides, SO2 has a 2:1 oxygen-to-sulfur ratio, and SO3 has a 3:1 ratio.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It is a fundamental concept for understanding the conservation of mass in reactions, and it involves calculations based on the balanced chemical equation.
When balancing chemical equations, such as the one involving dinitrogen pentoxide ((NO2)_{5}) and sulfur dioxide (SO2), stoichiometry helps us ensure that the number of atoms for each element is conserved across reactants and products. It guides us to deduce the right coefficients that will balance the equation. In our example, it's crucial to establish the correct amounts of sulfur trioxide (SO3) and nitrogen oxide (NO2) produced when given the amount of reactants. The exercise illustrates how the stoichiometric coefficients (2 for both products in the balanced equation) are determined through a step-by-step process, ensuring that not only individual atoms but also the total mass is balanced on both sides of the reaction equation.
Understanding stoichiometry allows students to predict the quantities of products formed from given reactants, which is invaluable for practical applications such as chemical manufacturing, where precise measurements are imperative for efficiency and safety.
When balancing chemical equations, such as the one involving dinitrogen pentoxide ((NO2)_{5}) and sulfur dioxide (SO2), stoichiometry helps us ensure that the number of atoms for each element is conserved across reactants and products. It guides us to deduce the right coefficients that will balance the equation. In our example, it's crucial to establish the correct amounts of sulfur trioxide (SO3) and nitrogen oxide (NO2) produced when given the amount of reactants. The exercise illustrates how the stoichiometric coefficients (2 for both products in the balanced equation) are determined through a step-by-step process, ensuring that not only individual atoms but also the total mass is balanced on both sides of the reaction equation.
Understanding stoichiometry allows students to predict the quantities of products formed from given reactants, which is invaluable for practical applications such as chemical manufacturing, where precise measurements are imperative for efficiency and safety.
Oxidation States
The concept of oxidation states, also known as oxidation numbers, is integral in the process of balancing chemical equations, particularly when dealing with compounds containing elements that can exist in multiple oxidation states.
Oxidation states indicate the degree of oxidation (loss of electrons) of an atom in a chemical compound. They are positive or negative numbers assigned to an atom based on a set of rules. For example, in the compound sulfur dioxide (SO2), sulfur has an oxidation state of +4, while each oxygen has an oxidation state of −2, reflecting the sharing of electrons between the atoms.
Determining the oxidation states helps clarify the changes in oxidation state that elements undergo during a reaction, thus guiding us in inferring the products of a reaction, particularly when elements form more than one compound, such as nitrogen in our equation possibly forming NO or NO2. In the provided example, nitrogen was deduced to be in the form of NO2, in which nitrogen has an oxidation state of +4 (consistent with the stoichiometrically balanced equation), rather than NO, where nitrogen would have an oxidation state of +2. Understanding and applying the concept of oxidation states is critical for predicting and balancing the chemical species that may arise in a particular reaction.
Oxidation states indicate the degree of oxidation (loss of electrons) of an atom in a chemical compound. They are positive or negative numbers assigned to an atom based on a set of rules. For example, in the compound sulfur dioxide (SO2), sulfur has an oxidation state of +4, while each oxygen has an oxidation state of −2, reflecting the sharing of electrons between the atoms.
Determining the oxidation states helps clarify the changes in oxidation state that elements undergo during a reaction, thus guiding us in inferring the products of a reaction, particularly when elements form more than one compound, such as nitrogen in our equation possibly forming NO or NO2. In the provided example, nitrogen was deduced to be in the form of NO2, in which nitrogen has an oxidation state of +4 (consistent with the stoichiometrically balanced equation), rather than NO, where nitrogen would have an oxidation state of +2. Understanding and applying the concept of oxidation states is critical for predicting and balancing the chemical species that may arise in a particular reaction.
Chemical Formulae
Chemical formulae represent the types and numbers of atoms in a substance and are essential tools in characterizing the components involved in a chemical reaction.
A chemical formula gives us a clear picture of the molecular or ionic composition of the substance, which is crucial when you're trying to balance a chemical reaction. In our exercise, we start with the reactants' formulae: dinitrogen pentoxide is given by the formula (NO2)5 and sulfur dioxide by SO2; while the products sulfur trioxide and nitrogen dioxide are represented as SO3 and NO2, respectively. These formulae explicitly indicate the proportions of each element in the molecules, which becomes the basis for balancing the reaction.
It's important to be able to correctly write and interpret these formulae as they dictate the stoichiometry of the equation. For example, the formula (NO2)5 signifies a compound with one nitrogen atom for every two and a half oxygen atoms, though such fractional stoichiometry does not exist in discrete molecules, hence the need to balance the chemical equation using whole-number coefficients. Understanding and writing correct chemical formulae is a foundational skill that enables the correct application of stoichiometry and elucidation of oxidation states in chemical reactions.
A chemical formula gives us a clear picture of the molecular or ionic composition of the substance, which is crucial when you're trying to balance a chemical reaction. In our exercise, we start with the reactants' formulae: dinitrogen pentoxide is given by the formula (NO2)5 and sulfur dioxide by SO2; while the products sulfur trioxide and nitrogen dioxide are represented as SO3 and NO2, respectively. These formulae explicitly indicate the proportions of each element in the molecules, which becomes the basis for balancing the reaction.
It's important to be able to correctly write and interpret these formulae as they dictate the stoichiometry of the equation. For example, the formula (NO2)5 signifies a compound with one nitrogen atom for every two and a half oxygen atoms, though such fractional stoichiometry does not exist in discrete molecules, hence the need to balance the chemical equation using whole-number coefficients. Understanding and writing correct chemical formulae is a foundational skill that enables the correct application of stoichiometry and elucidation of oxidation states in chemical reactions.
