Methanol (CH 3 OH) is used as a fuel in race cars. (d) Calculate the mass of CO 2 produced per kJ of heat emitted.

Write the balanced chemical equation for the combustion of methanol (CH 3 OH). The equation is CH 3 OH + 1.5 O 2 → CO 2 + 2 H 2 O.. Determine the molar mass of methanol (CH 3 OH) and carbon dioxide (CO 2 ).. Calculate the amount of heat released per mole of methanol combusted. This information can be found in thermodynamic tables or can be calculated from enthalpy changes.. Using stoichiometry, calculate the mass of CO 2 produced per mole of methanol combusted. This involves using the molar ratio from the balanced equation and the molar masses calculated in step 2.. Finally, calculate the mass of CO 2 produced per kJ of heat emitted by dividing the mass of CO 2 produced per mole of methanol by the heat released per mole of methanol, then multiplying by 1000 to convert from MJ to kJ.

Methanol (CH 3 OH) is used as a fuel in race cars. (d) Calculate the mass of CO 2 produced per kJ of heat emitted.

hey everyone in this example, we have the following reaction And we need to find the entropy of formation of 5.15 g of lead chloride. So we want to recognize whether our equation is balanced and based on our psyche aama tree and the coefficients. It's definitely a balanced equation. Our next step is to recognize that we are given the entropy of formation for reaction for our formation of lead chloride as negative 3 36 point okay, joules per mole and this is for one mole of our lead chloride. So we want to recognize that that comes from the coefficient one which is in front of our product lead chloride. So our next step is to first because we are given the amount in grams for lead chloride. We need to convert from grams to moles. So we want to start from 5.15 g of our lead chloride. And then we're going to go from grams to moles by recalling our molar mass for the compound. So when we find lead in group four a on our periodic tables, we see that it has a molar mass of 207.2 g per mole. And when we find chlorine in group seven a on the periodic table, We see that it has a molar mass of 35.4, 5 g per mole. Now recognize that in our formula, we have two moles of our Chlorine Atom. And so we're going to multiply this by two. So to get the total mass for the compound lead chloride, we're going to have these two masses added up together And we're going to have a total of 278.1 g per mole for our compound P BCL two. So we're going to plug that in. So we have to 78.1 g for one mole of our lead chloride. So this allows us to cancel out our units of grams leaving us with moles, which is what we want. And we're going to get a value equal to 0.01815 moles of our lead chloride. And actually I re I just need to rewrite this number. So it's actually 0.018 519 moles of our lead chloride. And so now we can calculate our anthem P A formation for our lead chloride For our 5.15 g of lead chloride. And we would get that that is equal to our entropy of formation for one mole, which is given as negative 3 36.0 Killer Jewels for one mole of lead chloride. And then we're multiplying this by our molds of our 5.15 g of our lead chloride which we found above. So we plugged that in as 0. moles of our lead chloride. So this allows us to cancel out most, leaving us with kayla jewels as our final unit, Which is definitely what we need for entropy of formation. And we get a value in our calculators equal to negative 6.22238. So we can round this to about 366 so that we have negative 6.22 kg joules as our final answer For the entropy of formation of our 5. g of our product, lead chloride. So I hope that everything we reviewed was clear. If you have any questions, please leave them down below and I will see everyone in the next practice video.

Ch.5 - Thermochemistry

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Brown 14th Edition

Ch.5 - Thermochemistry

Problem 80d

Chapter 5, Problem 80d

Methanol (CH₃OH) is used as a fuel in race cars. (d) Calculate the mass of CO₂ produced per kJ of heat emitted.

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Write the balanced chemical equation for the combustion of methanol (CH3OH). The equation is CH3OH + 1.5 O2 → CO2 + 2 H2O.

Determine the molar mass of methanol (CH3OH) and carbon dioxide (CO2).

Calculate the amount of heat released per mole of methanol combusted. This information can be found in thermodynamic tables or can be calculated from enthalpy changes.

Using stoichiometry, calculate the mass of CO2 produced per mole of methanol combusted. This involves using the molar ratio from the balanced equation and the molar masses calculated in step 2.

Finally, calculate the mass of CO2 produced per kJ of heat emitted by dividing the mass of CO2 produced per mole of methanol by the heat released per mole of methanol, then multiplying by 1000 to convert from MJ to kJ.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Combustion Reaction

A combustion reaction is a chemical process in which a substance (usually a hydrocarbon) reacts with oxygen to produce carbon dioxide and water, releasing energy in the form of heat. In the case of methanol (CH3OH), its combustion can be represented by the balanced equation: 2 CH3OH + 3 O2 → 2 CO2 + 4 H2O. Understanding this reaction is essential for calculating the amount of CO2 produced.

Stoichiometry

Stoichiometry is the quantitative relationship between the reactants and products in a chemical reaction. It allows us to determine how much of each substance is consumed or produced based on the balanced chemical equation. In this context, stoichiometry will help calculate the mass of CO2 produced per kJ of heat emitted by using the molar ratios from the combustion of methanol.

Energy Release in Combustion

The energy released during combustion is typically measured in kilojoules (kJ) and is derived from the breaking and forming of chemical bonds. The heat of combustion for methanol can be found in thermodynamic tables, which provides the amount of energy released per mole of methanol burned. This value is crucial for determining the mass of CO2 produced per kJ of heat emitted, as it links the energy output to the amount of fuel consumed.