Methane balanced chemical equation

Strategy Start by writing a balanced chemical equation for the reaction involved. Then use Equation 17.1 in combination with Table 17.1 to calculate the difference in entropy between products and reactants. For (b) note that you are asked to calculate AS° for one gram of methane. 

Sometimes we need to construct a balanced chemical equation from the description of a reaction. For example, methane, CH4, is the principal ingredient of natural gas (Fig. H.3). It burns in oxygen to form carbon dioxide and water, both formed initially as gases. To write the balanced equation for the reaction, we first write the skeletal equation ... 

Write the balanced chemical equation for the complete fluorination of methane to tetrafluoromethane. Using bond enthalpies, estimate the enthalpy of this reaction. The corresponding reaction using chlorine is much less exothermic. To what can this difference be attributed ... 

As another illustration of the use of Equation, we calculate the enthalpy of combustion of methane, the principal component of natural gas. We begin with the balanced chemical equation ... 

As usual, you need to begin with a balanced chemical equation. If a given reactant or product has a molar coefficient that is not 1, you need to multiply its AH°f by the same molar coefficient. This makes sense because the units of Aff°f are kj/mol. Consider, for example, the complete combustion of methane, CH4(g). 

Name another possible carbon-containing product from the incomplete combustion of methane. Write a balanced chemical equation for this reaction. 

The reactants shown schematically on the left represent methane, CH4, and water, HzO. Write out the full balanced chemical equation that is depicted. 

Q C99 Natural gas is mainly methane gas. If you have a natural gas furnace, stove, or water heater in your home, you must ensure that these appliances are always running at peak efficiency. In other words, the methane gas should undergo complete combustion so that carbon monoxide is not produced. Write a balanced chemical equation to show the complete combustion of methane gas. Write a second balanced equation to show the incomplete combustion of methane gas. 

To find the volume of a gaseous reactant or product in a reaction, you must know the balanced chemical equation for the reaction and the volume of at least one other gas involved in the reaction. Examine the reaction showing the combustion of methane, which takes place every time you light a Bunsen burner. 

How many dm3 of methane would react completely with 40 dm3 of oxygen gas when both substances are at STP, according to the balanced chemical equation shown here ... 

We are now ready to use chemical equations to calculate the relative amounts of substances involved in chemical reactions. Let us again consider the combustion of methane in excess oxygen. The balanced chemical equation for that reaction is... 

This interpretation tells us that one mole of methane reacts with two moles of oxygen to A balanced chemical equation may produce one mole of carbon dioxide and two moles of water. be interpreted in terms of moles of... 

The AHJ of a given compound is a physical constant and is independent of the process by which the compound is formed. Therefore, AHJ values are additive and can be calculated precisely for balanced chemical equations if all the necessary data are available. For example, it might be experimentally impossible to measure the A// of methane directly by calorimetry, but it can be calculated as the sum of the enthalpy for an equivalent reaction sequence, e.g ... 

Predict which of the two compounds, methane gas (GEI4) or methanal vapor (GH2O), has the greater molar enthalpy of combustion. Explain your answer. (Hint Write and compare the balanced chemical equations for the two combustion reactions.)... 

Natural gas consists primarily of methane, CH4(g). (a) Write a balanced chemical equation for the complete combustion of methane to produce C02(g) as the only carbon-containing product (b) Write a balanced chemical equation for the incomplete combustion of methane to produce CO(g) as the only carbon-containing product, (c) At 25 °C and 1.0 atm pressure, what is the minimum quantity of dry air needed to combust 1.0 L of CH4(g) completely to C02(g) ... 

Hydrogen cyanide (HCN) is extremely toxic, but it is used in the production of several important plastics. In the most common method for producing HCN, ammonia (NH3) and methane (CH4) react with oxygen (Oj) to give HCN and water. Write a balanced chemical equation for this reaction. 

The simplest combustible hydrocarbon—and therefore one of the simplest of all fuels—is methane, CH4. So the combustion of methane will provide a good place for us to begin our exploration of reaction stoichiometry. We start by writing a balanced chemical equation ... 

We start with the balanced chemical equation and use the stoichiometric coefficients to establish the mole ratio between methane and oxygen. Then, we can use that ratio to relate the amount of methane in the reaction to the amount of oxygen needed. 

X 10 ft of methane at atmospheric pressure and 25°C are oxidized to methanol, (a) What volume of methcmol is formed if the density of CH3OH is 0.791 g/L (b) Write balanced chemical equations for the oxidations of methane and methanol to CO ig) and H20(l). Calculate the total enthalpy change for complete combustion of the... 

A balanced chemical equation represents a chemical reaction. In this image, methane molecules combine with oxygen to form carbon dioxide and water. 

Carbon tetrachloride is used as an intermediate chemical in the manufacture of other chemicals. It is prepared in liquid form by reacting chlorine gas vwith methane gas. Hydrogen chloride gas is also formed in this reaction. Write the balanced chemical equation for the production of carbon tetrachloride. (Hint See Sample Problems C and D.)... 

Chemists determine the identity of the reactants and products of a reaction by experimental observation. For example, when methane (natural gas) is burned in the presence of sufficient oxygen gas, the products are always carbon dioxide and water. The identities (formulas) of the compounds must never he changed in balancing a chemical equation. In other words, the subscripts in a formula cannot be changed, nor can atoms be added to or subtracted from a formula. 

Figure 3.4 I The chemical reaction for the burning of methane (CH4) in oxygen illustrates the concept of atom balance for chemical equations. The equation is shown first in symbolic form, with each compound represented by its chemical formula. The individual molecules are pictured in the center row and then are broken down into their con-stiment atoms. The number of atoms of each element is the same on the left- and right-hand sides.

You can read the equation like this One molecule of methane gas, CH4(5), reacts with two molecules of oxygen gas, 02(g), to form one molecule of carbon dioxide gas, C02(g), and two molecules of water vapor, H20(g). The 2 in front of the oxygen gas and the 2 in front of the water vapor are called the reaction coefficients. They indicate the number of each chemical species that reacts or is formed. I show you how to figure out the value of the coefficients in the section Balancing Chemic il Reactions, later in the chapter. 

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