C2H4+3 O2->2 co2+2 H2O

If you start wit 45 grams of C2H4 how many grams of carbon dioxide will be produced?

C2H4 + 302 --> 2CO2 + 2H2O

1 : 2 mole ratio
m= 45g m= ?
M= 28.0 g/mol M= 44.0 g/mol
n= 45g/28.0 n= 2(1.61mol)
= 1.61 mol = 3.22 mol
m= (3.22 mol)
x (44.0 g/mol)
= 141.68 g

Therefore, 141.68 g of carbon dioxide with be produced.

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Well, let me put on my "chemistry clown" hat and calculate that for you!

According to the balanced equation, 1 mole of C2H4 produces 2 moles of CO2. The molar mass of C2H4 is approximately 28.05 g/mol, and the molar mass of CO2 is approximately 44.01 g/mol.

To find out how many moles of C2H4 you have in 45 grams, we divide the mass by the molar mass:

45 g / 28.05 g/mol = 1.60 mol of C2H4

Since 1 mole of C2H4 produces 2 moles of CO2, we multiply the number of moles of C2H4 by 2:

1.60 mol × 2 = 3.20 mol of CO2

And finally, to find the mass of 3.20 moles of CO2, we multiply the moles by the molar mass:

3.20 mol × 44.01 g/mol = 140.8 g of CO2

Therefore, if you start with 45 grams of C2H4, you'll end up with approximately 140.8 grams of CO2. That's a lot of carbon dioxide! I hope you're not planning on trapping it all in a balloon – you might float away!

To determine the amount of carbon dioxide produced, we need to calculate the molar mass of C2H4 and CO2 and then use stoichiometry. Here's the step-by-step solution:

Step 1: Calculate the molar mass of C2H4 and CO2.
The molar mass of C2H4 (ethylene) is calculated as:
2 carbon atoms (C) x 12.01 g/mol + 4 hydrogen atoms (H) x 1.008 g/mol
Molar mass of C2H4 = 28.05 g/mol

The molar mass of CO2 (carbon dioxide) is calculated as:
1 carbon atom (C) x 12.01 g/mol + 2 oxygen atoms (O) x 16.00 g/mol
Molar mass of CO2 = 44.01 g/mol

Step 2: Calculate the number of moles of C2H4.
Using the molar mass of C2H4, we can convert grams to moles:
45 g of C2H4 / 28.05 g/mol = 1.60 moles of C2H4

Step 3: Apply stoichiometry.
From the balanced equation, we know that 1 mole of C2H4 produces 2 moles of CO2.
So, 1.60 moles of C2H4 will produce:
1.60 moles C2H4 x (2 moles CO2 / 1 mole C2H4) = 3.20 moles of CO2

Step 4: Calculate the grams of CO2.
Using the molar mass of CO2, we can convert moles to grams:
3.20 moles of CO2 x 44.01 g/mol = 140.83 grams of CO2

Therefore, if you start with 45 grams of C2H4, you will produce 140.83 grams of carbon dioxide.

To determine the number of grams of carbon dioxide (CO2) produced in this chemical reaction, you need to use the given balanced equation and perform a stoichiometric calculation.

The balanced equation is: C2H4 + 3 O2 -> 2 CO2 + 2 H2O

First, calculate the molar mass of C2H4 (ethylene). C2H4 consists of two carbon atoms (C) with a molar mass of 12.01 g/mol each, and four hydrogen atoms (H) with a molar mass of 1.01 g/mol each.

Molar mass of C2H4 = (2 * molar mass of C) + (4 * molar mass of H)
= (2 * 12.01 g/mol) + (4 * 1.01 g/mol)
= 24.02 g/mol + 4.04 g/mol
= 28.06 g/mol

Using the molar mass of C2H4, you can calculate the number of moles present in 45 grams of C2H4.

Number of moles of C2H4 = Mass / Molar mass
= 45 g / 28.06 g/mol
= 1.60 mol (approximately)

According to the balanced equation, for every 1 mole of C2H4, 2 moles of CO2 are produced. Therefore, you can use the stoichiometry of the balanced equation to determine the number of moles of CO2 produced.

Number of moles of CO2 = (Number of moles of C2H4) * (Coefficient of CO2 / Coefficient of C2H4)
= 1.60 mol * (2 mol CO2 / 1 mol C2H4)
= 3.20 mol

Finally, calculate the mass of CO2 produced using the molar mass of CO2, which consists of one carbon (C) atom with a molar mass of 12.01 g/mol and two oxygen (O) atoms with a combined molar mass of 2 * 16.00 g/mol.

Molar mass of CO2 = (1 * molar mass of C) + (2 * molar mass of O)
= (1 * 12.01 g/mol) + (2 * 16.00 g/mol)
= 12.01 g/mol + 32.00 g/mol
= 44.01 g/mol

Mass of CO2 produced = (Number of moles of CO2) * (Molar mass of CO2)
= 3.20 mol * 44.01 g/mol
= 140.82 g (approximately)

Therefore, approximately 140.82 grams of carbon dioxide (CO2) will be produced from 45 grams of C2H4.