Question Video: Calculating the Molar Enthalpy Change for the Combustion of Methane | Nagwa Question Video: Calculating the Molar Enthalpy Change for the Combustion of Methane | Nagwa

# Question Video: Calculating the Molar Enthalpy Change for the Combustion of Methane Chemistry • First Year of Secondary School

When burned, 40.1 g of methane, (๐_(๐) = 16.04 g/mol), was found to raise the temperature of 10 kg of water by 53ยฐC. What is the molar enthalpy change, to the nearest whole number, for the combustion of methane? Take the specific heat capacity of water to be 4.2 J/gโยฐC.

04:05

### Video Transcript

When burned, 40.1 grams of methane, ๐ ๐ equals 16.04 grams per mole, was found to raise the temperature of 10 kilograms of water by 53 degrees Celsius. What is the molar enthalpy change, to the nearest whole number, for the combustion of methane? Take the specific heat capacity of water to be 4.2 joules per gram degrees Celsius.

Combustion is an example of an exothermic reaction, which is a type of reaction that releases energy. In a calorimetry experiment, methane can be combusted in a bomb calorimeter. As the reaction occurs, there is a transfer of thermal energy from the reaction system to the surrounding water. This thermal energy heats up the water, raising its temperature. One assumption we are making is that all the energy produced during the reaction only heats up the water and no energy is lost to the surrounding environment.

We can calculate the energy transferred during the chemical reaction by using the following equation, in which ๐ is the energy transferred in joules. ๐ is the mass in grams. ๐ is the specific heat capacity. And ฮ๐ก is the change in temperature in degrees Celsius. The specific heat capacity of a substance is the quantity of energy in joules required to raise the temperature of one gram of substance by one degree Celsius.

We are told to take the specific heat capacity of water to be 4.2 joules per gram degrees Celsius. We also know that the mass of water is 10 kilograms and the change in temperature of the water is 53 degrees Celsius.

Itโs important to note that the units for specific heat capacity include grams, but the mass of water is given in kilograms. Therefore, letโs convert the mass of water into grams by multiplying by 1000 grams per kilogram, which gives us 10000 grams.

We can now substitute the values into our equation to determine the value of ๐ to be 2226000 joules. This is a very large value to work with, so letโs convert it back into units of kilojoules by dividing by 1000. The value of ๐ is therefore 2226 kilojoules.

Now that we know how much heat was transferred to the water, we need to calculate the molar enthalpy change, which is the enthalpy change per mole of methane combusted. We can calculate the number of moles of methane by dividing the mass of methane by its molar mass. We are told that the mass of methane is 40.1 grams and the molar mass is 16.04 grams per mole. After dividing, we get the number of moles of methane. We can now calculate the molar enthalpy change by dividing the amount of energy transferred during the reaction, which was 2226 kilojoules, by the number of moles of methane.

Now that weโve calculated the molar enthalpy change, we need to round our answer to the nearest whole number. After rounding, we get 890 kilojoules per mole. Finally, we need to consider the sign this value should have. A positive sign is used for endothermic reactions to indicate that energy is absorbed by the system from the surroundings. A negative sign is used for exothermic reactions to indicate energy is released or lost from the system to the surroundings. A combustion reaction is an exothermic reaction, and we know heat was released to the water. So we need to use a negative sign.

Therefore, the molar enthalpy change for the combustion of methane is a negative 890 kilojoules per mole.

## Join Nagwa Classes

Attend live sessions on Nagwa Classes to boost your learning with guidance and advice from an expert teacher!

• Interactive Sessions
• Chat & Messaging
• Realistic Exam Questions