Carbon dioxide propane chemical reactions

One molecule (or mole) of propane reacts with five molecules (or moles) of oxygen to produce three molecules (or moles) or carbon dioxide and four molecules (or moles) of water. These numbers are called stoichiometric coefficients (v.) of the reaction and are shown below each reactant and product in the equation. In a stoichiometrically balanced equation, the total number of atoms of each constituent element in the reactants must be the same as that in the products. Thus, there are three atoms of C, eight atoms of H, and ten atoms of O on either side of the equation. This indicates that the compositions expressed in gram-atoms of elements remain unaltered during a chemical reaction. This is a consequence of the principle of conservation of mass applied to an isolated reactive system. It is also true that the combined mass of reactants is always equal to the combined mass of products in a chemical reaction, but the same is not generally valid for the total number of moles. To achieve equality on a molar basis, the sum of the stoichiometric coefficients for the reactants must equal the sum of v. for the products. Definitions of certain terms bearing relevance to reactive systems will follow next. 

F i ure 4.5 A combustion reaction. Here propane burns in air to give carbon dioxide and water. The balanced chemical equation informs us that one molecule of propane will combine with five molecules of oxygen to give three molecules of carbon dioxide and four molecules of water. Photo, C. D. Winters model, S. M. Young)... 

Diagram of a chemical reaction the combustion of propane with oxygen, resulting in carbon dioxide, water, and energy (as heat and light). This chemical reaction takes place in a camping stove as well as in certain welding torches. 

To develop the principles for dealing with the stoichiometry of reactions, we will consider the reaction of propane with oxygen to produce carbon dioxide and water. We will consider the question What mass of oxygen will react with 96.1 grams ofpropane In doing stoichiometry, the first thing we must do is write the balanced chemical equation for the reaction. In this case the balanced equation is... 

Your family may have a "gas grill" for outdoor cooking. Gas grills typically use bottled propane gas (CsHs), which burns in air (oxygen) to produce carbon dioxide gas and water vapor. Write the unbalanced chemical equation for this process. Gas grills should never be used indoors, however, because if the supply of oxygen is restricted, the products of the reaction tend to be water vapor and toxic carbon monoxide, instead of nontoxic carbon dioxide. Write the unbalanced chemical equation for this process. 

Propane, C3H8, is used as a fuel for gas barbecue grills, where it burns in a controlled fashion. But if a mixture of propane and air is ignited in a closed space, like a gas pipeline, an explosion can easily result. In either of these cases, the propane combines with oxygen, O2, to form carbon dioxide and water. Write a balanced chemical equation describing this reaction. 

We use units of kJ/mol for the heat of formation of a substance. But in writing the enthalpy change of a chemical reaction, we will use kJ as our preferred unit, not kj/mol. The reaction in this example illustrates why we do this. The value we calculated, AH° = -2219.9 kJ, is for a reaction in which one mole of propane reacts with five moles of oxygen to form three moles of carbon dioxide and four moles of water. So if we were to say -2219.9 kJ/mol, we would need to specify carefully which substance that mol refers to. We choose to write the AH value in kJ, with the understanding that it refers to the reaction as written. This is also dimension-ally consistent with Equation 9.12, provided that we treat the stoichiometric coefficients as carrying units of moles. You may see other texts that refer to values as per mole of reaction. ... 

For the smallest possible unit of this reaction, 1 propane molecule reacts with 5 oxygen molecules to produce 3 carbon dioxide molecules, and 4 water molecules, as shown by the respective numbers preceding the chemical formulas (there is understood to be a 1 in front of the CgHg). 

Consider the combustion of propane (CsHg). Commonly used as fuel in gas grills, propane (a gas) combines with oxygen (O2, a gas) to form carbon dioxide (CO2, a gas) and water (H2O, a liquid). Because each propane molecule contains three carbon atoms and because carbon dioxide (with one carbon atom) is the only product that contains carbon, each propane molecule that reacts must produce three CO2 molecules. Similarly, the eight hydrogen atoms from each propane molecule should produce four water molecules. These data give ten oxygen atoms in the products (from three CO2 and four H2O molecules), so there must be five O2 molecules in the reactants. Thus, the chemical equation for this reaction is... 

Practice Problem A Write and balance the chemical equation that represents the combustion of propane (i.e., the reaction of propane gas with oxygen gas to produce carbon dioxide gas and liquid water). 

Rame treatment is a thermal plasma method where exothermic reactions between oxygen and fuel gas create thermally activated radical atoms and molecules, such as, O, OH, NH, NO, and CN [87,88]. The most commonly used gases in flame treatment are propane (CjM ), natural gas or methane (CH ) and butane (C H,g). These gases mainly bum with atmospheric oxygen, producing water and carbon dioxide. The combustion is a complex process involving many chemical reactions, but it is well summarized by, Farris et al. [85] and Strobel et al. [89]. For example, the combustion reaction of propane is ... 

The reverse-flow chemical reactor (RFR) has been shown to be a potentially effective technique for many industrial chemical processes, including oxidation of volatile organic compounds such as propane, propylene, and carbon monoxide removal of nitrogen oxides sulfur dioxide oxidation or reduction production of synthesis gas methanol formation and ethylbenzene dehydration into styrene. An excellent introductory article in the topic is given by Eigenberger and Nieken on the effect of the kinetic reaction parameters, reactor size, and operating parameters on RFR performance. A detailed review that summarizes the applications and theory of RFR operation is given by Matros and Bunimovich. 

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