What is the standard enthalpy of combustion of peanuts?
Use the assumptions on contents in problem 100.
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The standard enthalpy of combustion of peanuts is the amount of heat released when one mole of peanuts is completely burned in excess oxygen under standard conditions (25°C and 1 atm pressure). The standard enthalpy of combustion can be determined experimentally or estimated using the calorific value of peanuts.
To determine the standard enthalpy of combustion experimentally, the peanuts would be burned in a bomb calorimeter, which is a sealed container surrounded by water. The heat released during the combustion reaction is absorbed by the water, and the temperature rise of the water can be measured. The standard enthalpy of combustion can then be calculated using the heat transfer equation (q = mcΔT), where q is the heat released, m is the mass of water, c is the specific heat capacity of water, and ΔT is the temperature rise.
Alternatively, the calorific value of peanuts can be used to estimate the standard enthalpy of combustion. The calorific value is the amount of heat produced per unit mass when the fuel is completely burned. For peanuts, the calorific value is typically around 30 megajoules per kilogram (MJ/kg). By using the molar mass of peanuts (~28 grams/mol), you can convert the calorific value to the standard enthalpy of combustion per mole of peanuts.
Therefore, the standard enthalpy of combustion of peanuts can be estimated to be approximately 30 megajoules per kilogram (MJ/kg) or calculated more precisely by performing experimental combustion reactions and measurements.
To find the standard enthalpy of combustion of peanuts, you can follow these steps:
1. Start by searching for the chemical formula of peanuts. Peanuts are primarily composed of fats, proteins, and carbohydrates, so you may want to search for the average chemical composition of peanuts.
2. Once you have the average chemical composition, calculate the molar mass of peanuts by summing the molar masses of the individual elements in their chemical formula.
3. Determine the balanced chemical equation for the combustion of peanuts. This equation shows the reactants (peanuts and oxygen) and the products (carbon dioxide, water, and any other byproducts).
4. Look for the standard enthalpy of formation values for each of the reactants and products involved in the combustion reaction. The standard enthalpy of formation represents the change in enthalpy when one mole of a compound is formed from its constituent elements in their standard states. These values can usually be found in chemical databases or textbooks.
5. Use the balanced chemical equation to determine the stoichiometry of the reaction. This means determining the coefficients that represent the ratio of reactants and products in the reaction.
6. Calculate the standard enthalpy change for the combustion reaction using the enthalpy of formation values. The enthalpy change is equal to the sum of the enthalpies of formation of the products minus the sum of the enthalpies of formation of the reactants, multiplying each by the stoichiometric coefficient.
7. The obtained value will give you the standard enthalpy of combustion of peanuts per mole of peanuts.