Fuels And Combustion

The relationship between the enthalpy ( $H$ ) and internal energy ( $U$ ) can be given by the following equation: $%5CDelta%20H%20%3D%20%5CDelta%20U%20%2B%20%5CDelta%20nRT$ Where: - $%5CDelta%20H$ is the change in enthalpy (given as -2546 kJ/mol), - $%5CDelta%20n$ is the change in the number of moles of gas in the reaction,
- $R$ is the gas constant ( $8.314%20%5C%2C%20J%20%5C%2C%20mol%5E%7B-1%7D%20%5C%2C%20K%5E%7B-1%7D$ ),
- $T$ is the temperature in Kelvin (298 K at 25°C). In the case of combustion, the combustion products (carbon dioxide and water) usually result in no change in the number of moles of gas ( $%5CDelta%20n%20%3D%200$ ).
Therefore, the internal energy change $%5CDelta%20U$ is equal to the enthalpy change $%5CDelta%20H$ : $%5CDelta%20U%20%3D%20%5CDelta%20H$ Hence, the internal energy change for the reaction is -2544.8 kJ/mol.

High-Yield Trend

Chapter Questions
1 MCQs

Official Solution

Fuels And Combustion

High-Yield Trend

Chapter Questions 1 MCQs

Official Solution

Chapter Questions
1 MCQs