Stearic acid (c18h36o2) is a fatty acid, a molecule with a long hydrocarbon chain and an organic acid group (cooh) at the end. it is used to make cosmetics, ointments, soaps, and candles and is found in animal tissue as part of many saturated fats. in fact, when you eat meat, you are ingesting some fats containing stearic acid. determine the latex: \deltaδhrxn for this combustion given the following information: latex: \deltaδhf of stearic acid = -948 kj/mol, latex: \deltaδhf of co2 = -394 kj/mol, latex: \deltaδhf of water = -242 kj/mol. calculate the heat (q) released in kj when 262 g of stearic acid reacts with 914.5 g of oxygen. enter a positive number to 0 decimal place.

There is 9671  Kj of heat released

Explanation:

Step 1: The balanced equation:

C18H36O2(s) + 26O2(g) --> 18CO2(g)+18H2O(g)

This means for 1 mole of C18H36O2 consumed there is 26 moles of O2 needed to produce 18 moles of CO2 and 18 moles of H2O.

Step 2: Calculate the heat of combustion

ΔH (combustion) = [18*(ΔHf of CO2) + 18*(ΔHf of H2O)] - [1*(ΔHf of C18H36O2) + 26*(ΔHf of O2)]

ΔH (combustion) = [18*(-394 kJ/mol) + 18*(-242 kJ/mol)] - [1*(-948 kJ/mol) + 26*(0 kJ/mol)]

ΔH (combustion) = [(-7092 kJ/mol) + (-4356 kJ/mol)] - (-948 kJ/mol)

= -10500 kJ/mol

ΔH (combustion) = heat released / number of moles of stearic acid

Step 3: Calculate moles of stearic acid

moles of stearic acid = mass / Molar mass of stearic acid

moles of stearic acid = 262g / 284.48 g/mole = 0.921 moles

Step 4: Calculate moles of oxygen

moles of O2 = 914.5 / 32g/mole

moles of O2 = 28.578125 moles

Stearic acid is the limiting reactant: it will completely react

There will react 26*0.921 mole = 23.946 mole of O2

This means there will remain 4.63 moles of O2

Step 5: Calculate heat released

q = (ΔH combustion) * (moles of stearic acid) = (-10500 kJ/mol) * (0.921 moles) = 9671 Kj

There is 9671  Kj of heat released

they vary. it used to be meat, grain, bread, candy, beverages, donuts, and fruits/vegetables. now they added exercise in.