CH3OH + CO → CH3COOH
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Word Equation
Methanol + Carbon Monoxide = Acetic Acid
One mole of
and one mole of
combine lớn sườn one mole of
Reactants
Methanol - CH3OH
Methyl Hydroxide Hydroxymethane Monohydroxymethane Colonial Spirit Columbian Spirit Spirit Of Wood Pyroxylic Spirit Methylol CH3OH Molar Mass CH3OH Oxidation Number
Carbon Monoxide - CO
Thermodynamics
Thermodynamics of the reaction can be calculated using a lookup table.
Is the Reaction Exothermic or Endothermic?
| CH3OH (g methanol) | 1 mol | -201.08304 kJ/mol | 201.08304 kJ |
|---|---|---|---|
| CO (g) | 1 mol | -110.54128 kJ/mol | 110.54128 kJ |
| CH3COOH (l acetic acid) | 1 mol | -484.13064 kJ/mol | -484.13064 kJ |
| ΣΔH°f(reactants) | -311.62432 kJ | ||
| ΣΔH°f(products) | -484.13064 kJ | ||
| ΔH°rxn | -172.50632 kJ | ||
ΣΔH°f(reactants) > ΣΔH°f(products), sánh CH3OH + CO = CH3COOH is exothermic (releases heat).
Is the Reaction Exoentropic or Endoentropic?
ΔS = Sproducts - Sreactants. If ΔS < 0, it is exoentropic. If ΔS > 0, it is endoentropic.
| CH3OH (g methanol) | 1 mol | 239.70136 J/(mol K) | -239.70136 J/K |
|---|---|---|---|
| CO (g) | 1 mol | 197.9032 J/(mol K) | -197.9032 J/K |
| CH3COOH (l acetic acid) | 1 mol | 159.8288 J/(mol K) | 159.8288 J/K |
| ΣΔS°(reactants) | 437.60456 J/K | ||
| ΣΔS°(products) | 159.8288 J/K | ||
| ΔS°rxn | -277.77576 J/K | ||
ΣΔS°(reactants) > ΣΔS°(products), sánh CH3OH + CO = CH3COOH is exoentropic (decrease in entropy).
Is the Reaction Exergonic or Endergonic?
ΔG = Gproducts - Greactants. If ΔG < 0, it is exergonic. If ΔG > 0, it is endergonic.
| CH3OH (g methanol) | 1 mol | -162.42288 kJ/mol | 162.42288 kJ |
|---|---|---|---|
| CO (g) | 1 mol | -137.27704 kJ/mol | 137.27704 kJ |
| CH3COOH (l acetic acid) | 1 mol | -389.9488 kJ/mol | -389.9488 kJ |
| ΣΔG°(reactants) | -299.69992 kJ | ||
| ΣΔG°(products) | -389.9488 kJ | ||
| ΔG°rxn | -90.24888 kJ | ||
ΣΔG°(reactants) > ΣΔG°(products), sánh CH3OH + CO = CH3COOH is exergonic (releases energy).
Reaction Expressions
Kc or Q = ( [CH3COOH] ) / ( [CH3OH] [CO] )
(assuming all reactants and products are aqueous. substitutue 1 for any solids/liquids, and Psubstance for gases.)
rate = -(Δ[CH3OH] / Δt) = -(Δ[CO] / Δt) = (Δ[CH3COOH] / Δt)
(assuming constant volume in a closed system and no accumulation of intermediates or side products)
Instructions
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To balance a chemical equation, enter an equation of a chemical reaction and press the Balance button. The balanced equation will appear above.
- Use uppercase for the first character in the element and lowercase for the second character. Examples: Fe, Au, Co, Br, C, O, N, F.
- Ionic charges are not yet supported and will be ignored.
- Replace immutable groups in compounds lớn avoid ambiguity. For example, C6H5C2H5 + O2 = C6H5OH + CO2 + H2O will not be balanced, but XC2H5 + O2 = XOH + CO2 + H2O will.
- Compound states [like (s) (aq) or (g)] are not required.
- You can use parenthesis () or brackets [].
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Balance CH3OH + CO = CH3COOH Using the Algebraic Method
To balance the equation CH3OH + CO = CH3COOH 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 With a Variable
Label each compound (reactant or product) in the equation with a variable lớn represent the unknown coefficients.
a CH3OH + b CO = c CH3COOH
Create a System of Equations
Create an equation for each element (C, H, O) where each term represents the number of atoms of the element in each reactant or product.
C: 1a + 1b = 2c H: 4a + 0b = 4c O: 1a + 1b = 2c
Solve For All Variables
Use substitution, Gaussian elimination, or a calculator lớn solve for each variable.
- 1a + 1b - 2c = 0
- 4a - 4c = 0
- 1a + 1b - 2c = 0
Use your graphing calculator's rref() function (or an online rref calculator) lớn convert the following matrix into reduced row-echelon-form:
[ 1 1 -2 0] [ 4 0 -4 0] [ 1 1 -2 0]
The resulting matrix can be used lớn determine the coefficients. In the case of a single solution, the last column of the matrix will contain the coefficients.
Simplify the result lớn get the lowest, whole integer values.
- a = 1 (CH3OH)
- b = 1 (CO)
- c = 1 (CH3COOH)
Substitute Coefficients and Verify Result
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.
CH3OH + CO = CH3COOH
Reactants Products C 2 2 ✔️ H 4 4 ✔️ O 2 2 ✔️ Since there is an equal number of each element in the reactants and products of CH3OH + CO = CH3COOH, the equation is balanced.
Balance CH3OH + CO = CH3COOH Using Inspection
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 over of a chemical reaction as at the beginning. To be balanced, every element in CH3OH + CO = CH3COOH 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 lớn balance one element at a time until both sides are equal and the chemical equation is balanced.
1. Count the number of each element on the left and right hand sides
| Reactants (Left Hand Side) | Products (Right Hand Side) | |||||
|---|---|---|---|---|---|---|
| Reactants | Products | |||||
| CH3OH | CO | Total | CH3COOH | Total | ||
| C | 1 | 1 | 2 | 2 | 2 | ✔️ |
| H | 4 | 4 | 4 | 4 | ✔️ | |
| O | 1 | 1 | 2 | 2 | 2 | ✔️ |
The number of atoms of each element on both sides of CH3OH + CO = CH3COOH is equal which means that the equation is already balanced and no additional work is needed.
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