Ethane (C2H6) boils at a lower temperature of 84 °C compared to ethane (C2H4) at 88.6 °C because ethane has a higher molecular weight and stronger intermolecular forces. The stronger intermolecular forces in ethane require more energy to overcome, resulting in a higher boiling point. Ethane, on the other hand, has weaker intermolecular forces due to its smaller molecular size, leading to a lower boiling point. Therefore, the difference in boiling points between ethane and ethane can be attributed to the differences in their molecular weights and intermolecular forces. **

In the reaction between ethane and iodine, one possible product that can be formed is diiodoethane (also known as 1,2-diiodoethane). This compound is formed when one iodine atom replaces one of the hydrogen atoms in ethane. Additionally, if the reaction continues, other derivatives such as triiodoethane (also known as 1,1,2-triiodoethane) and tetraiodoethane (also known as 1,1,2,2-tetraiodoethane) can also be formed by further substitution of hydrogen atoms with iodine atoms. **

Ethene and ethane are both hydrocarbons, meaning they are composed of carbon and hydrogen atoms. They are both aliphatic compounds, which means they have straight chain structures. Additionally, both ethene and ethane are colorless and odorless gases at room temperature and pressure. **

Ethanol is a liquid at room temperature because it has stronger intermolecular forces of attraction compared to ethane. Ethanol molecules can form hydrogen bonds with each other, which results in a higher boiling point and a liquid state. On the other hand, ethane molecules are nonpolar and can only experience weaker van der Waals forces, leading to a lower boiling point and a gaseous state at room temperature. **

Ethane is a hydrocarbon with the chemical formula C2H6, while ethanol is an alcohol with the chemical formula C2H5OH. Ethane is a simple alkane, while ethanol is a type of alcohol that contains a hydroxyl group. Ethanol is commonly used as a solvent, fuel, and in alcoholic beverages, while ethane is primarily used as a fuel and in the production of ethylene. **

The complete combustion of ethane occurs when it reacts with oxygen in the presence of a flame or spark. The chemical equation for the complete combustion of ethane is: C2H6 + 7/2O2 → 2CO2 + 3H2O. This means that one molecule of ethane reacts with 7/2 molecules of oxygen to produce two molecules of carbon dioxide and three molecules of water. This reaction releases a large amount of heat and light, making it a highly exothermic process. **

The bromination of ethane is carried out by reacting ethane with bromine gas in the presence of a catalyst such as iron or aluminum. The reaction takes place at room temperature and atmospheric pressure. The bromine molecule breaks apart and adds to the carbon-carbon double bond in ethane, resulting in the formation of 1,2-dibromoethane. This reaction is an example of an addition reaction, where the bromine atoms add across the double bond of ethane. **

The chlorination of ethane is carried out by reacting ethane with chlorine gas in the presence of ultraviolet light or heat. This reaction results in the substitution of one or more hydrogen atoms in ethane with chlorine atoms, forming chloroethane and other chlorinated products. The reaction is typically carried out in the gas phase or in the presence of a solvent such as carbon tetrachloride. The process is important for the production of various chlorinated compounds used in the chemical industry. **