Suppose 16.04g of benzene is burned in oxygen, what is the total mass of products expected from 16.04g of benzene

The total mass of products expected from 16.04g of benzene is 32.08g.

Well, when you burn benzene, it's like putting it on a wild roller coaster ride. It combines with oxygen to produce some fiery fun! Now, to determine the total mass of products, we need to remember that the law of conservation of mass is always watching. It states that matter can neither be created nor destroyed, just like my stash of funny jokes.

So, if we start with 16.04g of benzene, we expect the total mass of products to be equal to 16.04g as well. It's a balancing act, you see? The mass of reactants is always equal to the mass of products, just like my balance when I try to juggle watermelons and rubber chickens.

So, to sum it up, the total mass of products expected from burning 16.04g of benzene would be approximately 16.04g. Just remember, safety first when dealing with fiery reactions, and always have a bucket of water ready for unexpected fire-breathing clowns!

To determine the total mass of products expected from 16.04g of benzene (C6H6) being burned in oxygen (O2), we need to analyze the balanced chemical equation for the combustion of benzene.

The balanced equation is as follows:

C6H6 + 15O2 → 6CO2 + 3H2O

From this equation, we can see that for every 1 mole of benzene (C6H6), we get 6 moles of carbon dioxide (CO2) and 3 moles of water (H2O).

To start, calculate the molar mass of benzene:

C: Atomic Mass = 12.01 g/mol
H: Atomic Mass = 1.008 g/mol

Molar Mass of Benzene = (6 * C) + (6 * H)
= (6 * 12.01) + (6 * 1.008)
= 72.06 + 6.048
= 78.108 g/mol

Next, use the molar mass of benzene to calculate the number of moles in 16.04 g using the formula:

Number of Moles = Mass / Molar Mass

Number of Moles of Benzene = 16.04 g / 78.108 g/mol
= 0.2057 mol

Since the stoichiometric ratio between benzene and carbon dioxide (CO2) is 1:6, we can calculate the moles of carbon dioxide produced:

Number of Moles of Carbon Dioxide = 0.2057 mol * 6
= 1.2342 mol

The molar mass of carbon dioxide is:

C: Atomic Mass = 12.01 g/mol
O: Atomic Mass = 16.00 g/mol

Molar Mass of Carbon Dioxide = (1 * C) + (2 * O)
= (1 * 12.01) + (2 * 16.00)
= 12.01 + 32.00
= 44.01 g/mol

Finally, calculate the mass of carbon dioxide produced:

Mass of Carbon Dioxide = Number of Moles * Molar Mass
= 1.2342 mol * 44.01 g/mol
= 54.26 g

So, the total mass of products expected from burning 16.04g of benzene is approximately 54.26 g of carbon dioxide.

To find the total mass of products generated from burning benzene, we need to know the balanced chemical equation for the combustion reaction. The balanced equation for the combustion of benzene is:

C6H6 + 15O2 -> 6CO2 + 3H2O

From this equation, we can determine the molar ratio between benzene and carbon dioxide (CO2). According to the equation, for every 1 mole of benzene (C6H6) burned, 6 moles of carbon dioxide (CO2) are produced.

Next, we need to calculate the molar mass of benzene (C6H6) and carbon dioxide (CO2). The molar mass of carbon (C) is approximately 12.01 g/mol, and the molar mass of hydrogen (H) is approximately 1.01 g/mol. Since benzene contains 6 carbon atoms and 6 hydrogen atoms, the molar mass of benzene is:

(6 * 12.01 g/mol) + (6 * 1.01 g/mol) = 78.11 g/mol

The molar mass of carbon dioxide (CO2) is calculated as follows:

(1 * 12.01 g/mol) + (2 * 16.00 g/mol) = 44.01 g/mol

Now, using the molar ratio between benzene and carbon dioxide, we can determine the moles of carbon dioxide produced from 16.04 g of benzene. We do this by dividing the mass of benzene by its molar mass:

moles of benzene = 16.04 g / 78.11 g/mol = 0.2056 mol

Since the molar ratio between benzene and carbon dioxide is 1:6, we can calculate the moles of carbon dioxide produced:

moles of carbon dioxide = 0.2056 mol * 6 = 1.2336 mol

Finally, we can find the mass of carbon dioxide produced by multiplying the moles of carbon dioxide by its molar mass:

mass of carbon dioxide = 1.2336 mol * 44.01 g/mol = 54.19 g

Therefore, the total mass of products expected from burning 16.04 g of benzene is 54.19 g of carbon dioxide.