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CO H2 CH3-CH=CH2 = C3H7CHO | Chemical Equation Balancer

1-Propene; Propylene; Propene; NCI-C-50077; R-1270 = Butanal; 1-Butanal; Butyraldehyde; n-Butyraldehyde; Butyric aldehyde; NCI-C-56291; Butyral; Butal; Butaldehyde; Butane-1-one; 3-Methylpropanal; 1-Butanone; Butanaldehyde

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Searching in our database with more than 5552 chemical substances

CO



cacbon oxit


carbon monoxide



Atomic_weight (g/mol) 28.0101


Density of solid (kg/m3) 1145


Boiling Point (°C) -192


Melting point (°C) -205

H2



hidro


hydrogen



Atomic_weight (g/mol) 2.01588 ± 0.00014


Density of solid (kg/m3) 70


Boiling Point (°C) -252


Melting point (°C) -259


Electron negativity 2


First Ionisation Energy 1312

CH3-CH=CH2

short form



1-Propen


1-Propene; Propylene; Propene; NCI-C-50077; R-1270


C3H7CHO

short form C4H8O



Butanal


Butanal; 1-Butanal; Butyraldehyde; n-Butyraldehyde; Butyric aldehyde; NCI-C-56291; Butyral; Butal; Butaldehyde; Butane-1-one; 3-Methylpropanal; 1-Butanone; Butanaldehyde



Atomic_weight (g/mol) 72.1057

Combination reaction

Also known as a synthesis reaction. One kind of frequently occurring combination reaction is the reaction of an element with oxygen to form an oxide. Under certain conditions, metals and nonmetals both react readily with oxygen. Once ignited, magnesium reacts rapidly and dramatically, reacting with oxygen from the air to create a fine magnesium oxide powder.

2Mg + O2 → 2MgO 3Cl2 + 2P → 2PCl3 H2SO4 + 2NH3 → (NH4)2SO4 Cl2 + Mg → MgCl2 2Al + 3Br2 → 2AlBr3 BaO + H2O → Ba(OH)2 H2O + ZnO → Zn(OH)2 View All Combination reaction
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Decomposition reaction

Many decomposition reactions involve heat , light, or electricity to input energy. Binary compounds are compounds which consist of only two elements. The simplest sort of reaction to decomposition is when a binary compound breaks down into its elements. Mercury (II) oxide, a red solid, decomposes to form mercury and oxygen gas when heated. Also, a reaction is regarded as a decomposition reaction even if one or more of the products are still a compound. A metal carbonate breaks down to form a metal oxide and carbon dioxide gas. Calcium carbonate for example decomposes into calcium oxide and carbon dioxide.

MgCO3 → MgO + CO2 3HClO3 → H2O + 2ClO2 + HClO4 Fe2(SO4)3 → Fe2O3 + 3SO3 CaCl2 → Ca + Cl2 C2H5OH → C2H4 + H2O 2HCl → Cl2 + H2 H2CO3 → H2O + CO2 View All Decomposition reaction
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Oxidation-reduction reaction

An oxidation-reduction (redox) reaction is a type of chemical reaction that involves a transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. Redox reactions are common and vital to some of the basic functions of life, including photosynthesis, respiration, combustion, and corrosion or rusting.

Cl2 + H2O + H2SO3 → H2SO4 + 2HCl 3H2SO4 + 2KMnO4 + 5K2SO3 → 3H2O + 2MnSO4 + 6K2SO4 2Cu2O + Cu2S → 2Cu + SO2 2CO2 + 2Na2O2 → 2Na2CO3 + O2 Cl2 + 2HI → 2HCl + I2 NH4HCO3 → H2O + NH3 + CO2 2C + Na2SO4 → Na2S + 2CO2 View All Oxidation-reduction reaction
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Single-replacement reaction

A + BC → AC + B Element A is a metal in this general reaction and replaces element B, a metal in the compound as well. If the replacement element is a non-metal, it must replace another non-metal in a compound, and it becomes the general equation. Many metals easily react with acids, and one of the reaction products when they do so is hydrogen gas. Zinc reacts to the aqueous zinc chloride and hydrogen with hydrochloride acid (see figure below).

Fe + 2HCl → FeCl2 + H2 3Cl2 + 2NH3 → 6HCl + N2 Cl2 + 2NaI → I2 + 2NaCl 2HCl + Mg → H2 + MgCl2 2Al + 3CuCl2 → 2AlCl3 + 3Cu H2O + CH3COCl → CH3COOH + HCl Al(OH)3 + NaOH → 2H2O + NaAlO2 View All Single-replacement reaction
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Double-replacement reaction

AB + CD → AD + CB A and C are positive charged cations in this reaction, while B and D are negative charged anions. Double-replacement reactions typically occur in aqueous solution between the compounds. To cause a reaction, one of the products is usually a solid precipitate, a gas, or a molecular compound like water. A precipitate forms in a double-replacement reaction when the cations from one reactant combine to form an insoluble ionic compound with the anions from the other reactant. The following reaction occurs when aqueous solutions of potassium iodide and lead ( II) nitrate are blended.

2H2SO4 + ZnS → 2H2S + ZnSO4 Mg(NO3)2 + 2NaOH → Mg(OH)2 + 2NaNO3 3Ba(NO3)2 + Fe2(SO4)3 → 2Fe(NO3)3 + 3BaSO4 2HBr + SOCl2 → 2HCl + SOBr2 2HCl + K2SiO3 → 2KCl + H2SiO3 H2SO4 + 2NH4NO3 → (NH4)2SO4 + 2HNO3 10CH3COCH3 + 12KMnO4 + 36KHSO4 → 10CH3COOH + 28H2O + 12MnSO4 + 24K2SO4 + 5CO2 View All Double-replacement reaction
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Equations with C3H7CHO as product

Butanal; 1-Butanal; Butyraldehyde; n-Butyraldehyde; Butyric aldehyde; NCI-C-56291; Butyral; Butal; Butaldehyde; Butane-1-one; 3-Methylpropanal; 1-Butanone; Butanaldehyde

CO + H2 + CH3-CH=CH2 → C3H7CHO View all equations with C3H7CHO as product
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