Nitric Oxide (Radical) + Dioxygen = Nitrogen Dioxide
NO + O2 = NO2 is a Synthesis reaction where two moles of
Thermodynamics of the reaction can be calculated using a lookup table.
NO (g) | 2 mol | 90.24888 kJ/mol | -180.49776 kJ |
---|---|---|---|
O2 (g) | 1 mol | 0 kJ/mol | -0 kJ |
NO2 (g) | 2 mol | 33.17912 kJ/mol | 66.35824 kJ |
ΣΔH°f(reactants) | 180.49776 kJ | ||
ΣΔH°f(products) | 66.35824 kJ | ||
ΔH°rxn | -114.13952 kJ |
ΔS = Sproducts - Sreactants. If ΔS < 0, it is exoentropic. If ΔS > 0, it is endoentropic.
NO (g) | 2 mol | 210.651848 J/(mol K) | -421.303696 J/K |
---|---|---|---|
O2 (g) | 1 mol | 205.028552 J/(mol K) | -205.028552 J/K |
NO2 (g) | 2 mol | 239.9524 J/(mol K) | 479.9048 J/K |
ΣΔS°(reactants) | 626.332248 J/K | ||
ΣΔS°(products) | 479.9048 J/K | ||
ΔS°rxn | -146.427448 J/K |
ΔG = Gproducts - Greactants. If ΔG < 0, it is exergonic. If ΔG > 0, it is endergonic.
NO (g) | 2 mol | 86.56696 kJ/mol | -173.13392 kJ |
---|---|---|---|
O2 (g) | 1 mol | 0 kJ/mol | -0 kJ |
NO2 (g) | 2 mol | 51.29584 kJ/mol | 102.59168 kJ |
ΣΔG°(reactants) | 173.13392 kJ | ||
ΣΔG°(products) | 102.59168 kJ | ||
ΔG°rxn | -70.54224 kJ |
To balance the equation NO + O2 = NO2 using the algebraic method step-by-step, you must have experience solving systems of linear equations. The most common methods are substitution/elimination and linear algebra, but any similar method will work.
Label each compound (reactant or product) in the equation with a variable to represent the unknown coefficients.
a NO + b O2 = c NO2
Create an equation for each element (N, O) where each term represents the number of atoms of the element in each reactant or product.
N: 1a + 0b = 1c O: 1a + 2b = 2c
Use substitution, Gaussian elimination, or a calculator to solve for each variable.
Use your graphing calculator's rref() function (or an online rref calculator) to convert the following matrix into reduced row-echelon-form:
[ 1 0 -1 0] [ 1 2 -2 0]
Simplify the result to get the lowest, whole integer values.
Count the number of atoms of each element on each side of the equation and verify that all elements and electrons (if there are charges/ions) are balanced.
2 NO + O2 = 2 NO2N | 2 | 2 | ✔️ |
---|---|---|---|
O | 4 | 4 | ✔️ |
The law of conservation of mass states that matter cannot be created or destroyed, which means there must be the same number atoms at the end of a chemical reaction as at the beginning. To be balanced, every element in NO + O2 = NO2 must have the same number of atoms on each side of the equation. When using the inspection method (also known as the trial-and-error method), this principle is used to balance one element at a time until both sides are equal and the chemical equation is balanced.
Reactants (Left Hand Side) | Products (Right Hand Side) | |||||
---|---|---|---|---|---|---|
Reactants | Products | |||||
NO | O2 | Total | NO2 | Total | ||
N | 1 | 1 | 1 | 1 | ✔️ | |
O | 1 | 2 | 3 | 2 | 2 | ❌ |
For each element that is not equal, try to balance it by adding more of it to the side with less. Sometimes there may be multiple compounds with that element on one side, so you'll need to use your best judgement and be prepared to go back and try the other options.
Reactants | Products | ||
---|---|---|---|
N | 1 | 2 | ❌ |
O | 3 | 4 | ❌ |
Reactants | Products | ||
---|---|---|---|
N | 2 | 2 | ✔️ |
O | 4 | 4 | ✔️ |
Since there are an equal number of atoms of each element on both sides, the equation is balanced.
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