Methane (CH4) is the major component of natural gas. 2.5 moles of methane were placed in a commercial colorimeter and subjected to a combustion reaction. The reaction released 2800 kJ of energy.

Compare this energy value to the energy values of paraffin and diethylene glycol. Is methane a good choice as a fuel?

To compare the energy values of different substances, we need to calculate the energy released per mole of the substance. By doing so, we can determine which substance has a higher energy content and evaluate if methane is a good choice as a fuel.

First, let's calculate the energy released per mole of methane. We know that 2.5 moles of methane released 2800 kJ of energy. To find the energy released per mole, we divide the total energy released by the number of moles:

Energy released per mole of methane = 2800 kJ / 2.5 moles ≈ 1120 kJ/mol

Now, we need to compare this value to the energy values of paraffin and diethylene glycol, which are commonly used fuels.

Paraffin, also known as hydrocarbon wax, has the molecular formula C25H52. The combustion of paraffin releases approximately 42 kJ/g.

To calculate the energy released per mole of paraffin, we need to know its molar mass. The molar mass of paraffin can be calculated by adding up the atomic masses of its constituent atoms:

Molar mass of paraffin = (25 mol of carbon × 12.01 g/mol) + (52 mol of hydrogen × 1.01 g/mol)
≈ 300.78 g/mol

Next, we convert the energy released per gram to the energy released per mole:

Energy released per mole of paraffin = (42 kJ/g) / (300.78 g/mol)
≈ 0.14 kJ/mol

Diethylene glycol, with the chemical formula C4H10O3, is a common industrial solvent. Its combustion releases approximately 23.5 kJ/g.

Again, we need to calculate the molar mass of diethylene glycol:

Molar mass of diethylene glycol = (4 mol of carbon × 12.01 g/mol) + (10 mol of hydrogen × 1.01 g/mol) + (3 mol of oxygen × 16.00 g/mol)
≈ 106.14 g/mol

Now, we determine the energy released per mole of diethylene glycol:

Energy released per mole of diethylene glycol = (23.5 kJ/g) / (106.14 g/mol)
≈ 0.22 kJ/mol

Comparing the calculated values:

Energy released per mole of methane: 1120 kJ/mol
Energy released per mole of paraffin: 0.14 kJ/mol
Energy released per mole of diethylene glycol: 0.22 kJ/mol

From these calculations, it is evident that methane releases significantly more energy per mole compared to both paraffin and diethylene glycol. Therefore, methane is indeed a good choice as a fuel due to its high energy content.

Please note that the values of energy released per mole used in this explanation are approximate and can vary depending on the specific conditions and sources considered.

To compare the energy value of methane to paraffin and diethylene glycol, we will need to calculate their respective energy values per mole.

The balanced chemical equation for the combustion of methane is as follows:
CH4 + 2O2 -> CO2 + 2H2O

From the balanced equation, we can determine that 1 mole of methane (CH4) produces 1 mole of carbon dioxide (CO2) and 2 moles of water (H2O) during combustion.

To calculate the energy released per mole of methane, we divide the given energy (2800 kJ) by the number of moles of methane (2.5 moles) used in the reaction:
Energy per mole of methane = 2800 kJ/2.5 moles = 1120 kJ/mol

Now, let's compare this energy value to the energy values of paraffin and diethylene glycol.

Paraffin, which is a mixture of hydrocarbons, has an average energy value of around 42 kJ/g. To convert this value to energy per mole, we need to determine the molar mass of paraffin. The molar mass of paraffin can vary depending on the specific composition, but let's assume an average molar mass of 200 g/mol for our comparison:
Energy per mole of paraffin = (42 kJ/g) x (200 g/mol) = 8400 kJ/mol

Diethylene glycol (C4H10O3) has a molar mass of approximately 106 g/mol. Its combustion reaction can be written as:
C4H10O3 + 6O2 -> 4CO2 + 5H2O

Using the stoichiometry of the reaction, we can determine that 1 mole of diethylene glycol produces 4 moles of carbon dioxide and 5 moles of water during combustion.

Assuming that the combustion of diethylene glycol also releases 2800 kJ of energy, the energy released per mole can be calculated as:
Energy per mole of diethylene glycol = 2800 kJ/1 mole = 2800 kJ/mol

Based on the calculated energy values per mole of methane, paraffin, and diethylene glycol, we can see that methane has the lowest energy value at 1120 kJ/mol. Compared to paraffin (8400 kJ/mol) and diethylene glycol (2800 kJ/mol), it can be concluded that methane is a poor choice as a fuel if we consider only the energy content.

So you know 2.5 mols CH$ releases 2800 kJ of energy. (By the way that is calorimeter).

Look up the energy values for paraffin and the glycol and compare them. That's all there is to it. You can find that information on Google.