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Video instructions and help with filling out and completing Who Form 2220 Calculator

Instructions and Help about Who Form 2220 Calculator

In this video, we'll calculate the enthalpy of a chemical reaction process. The specific reaction we'll be analyzing is the combustion of butane gas. Butane, being a hydrocarbon, contains a significant amount of potential energy. When it reacts with oxygen, this energy is released in an exothermic process. The products of this reaction are carbon dioxide and water. Due to the substantial energy release, we can record this information. To calculate the exact amount of energy released in this process, we need to consider the change in enthalpy for the combustion of butane. The value for this is 2877.5 kilojoules per mole. This value tells us how much energy is released when one mole of butane is burned. The negative sign associated with this value indicates that it is an exothermic process, where the energy content of the products is lower than that of the reactants. By analyzing an energy diagram, we can observe that the energy content of butane is higher compared to the energy content of the products, carbon dioxide and water. Therefore, when we calculate Delta H (the change in enthalpy), it will be a negative value once again indicating an exothermic reaction. To solve this problem, we need to dimensional analysis. Firstly, we must convert the mass of butane being combusted from 0.13 grams to moles. For this conversion, we require the molar mass of butane, which is 58.14 grams per mole. The molar mass is determined by using the subscripts from the chemical formula. In this case, carbon has four atoms, so we calculate 12.01 (mass of carbon) multiplied by 4, giving us 48.04. Hydrogen, with 10 atoms, is calculated by multiplying 1.01 (mass of hydrogen) by 10, leading to 10.1. Next, we convert from grams of butane to moles of butane using the calculated value. We will...