In the formula 2C4H10+13O2=10H2O+8CO2 whats the mass of butane needed to produce 79.7g of carbon dioxide.

To calculate the mass of butane needed to produce 79.7g of carbon dioxide (CO2), we need to use stoichiometry and the balanced chemical equation.

The balanced chemical equation for the combustion of butane (C4H10) is:

2C4H10 + 13O2 -> 10H2O + 8CO2

From this equation, we can see that for every 8 moles of CO2 produced, we need 2 moles of C4H10.

Now, let's calculate the moles of CO2 produced:

Molar mass of CO2 = 12.01 g/mol (carbon) + 2 * 16.00 g/mol (oxygen) = 44.01 g/mol

Moles of CO2 = Mass of CO2 / Molar mass of CO2
= 79.7 g / 44.01 g/mol
≈ 1.81 mol

Since the molar ratio of C4H10 to CO2 is 2:8, we can set up a proportion to determine the moles of C4H10 needed:

(2 mol C4H10 / 8 mol CO2) = (x mol C4H10 / 1.81 mol CO2)

Solving for x:
x mol C4H10 = (2 mol C4H10 / 8 mol CO2) * 1.81 mol CO2
= 0.4525 mol C4H10

Now, let's calculate the mass of butane needed:

Molar mass of C4H10 = 4 * 12.01 g/mol (carbon) + 10 * 1.01 g/mol (hydrogen)
= 58.12 g/mol

Mass of C4H10 = Moles of C4H10 * Molar mass of C4H10
= 0.4525 mol * 58.12 g/mol
≈ 26.28 g

Therefore, approximately 26.28 grams of butane (C4H10) are needed to produce 79.7 grams of carbon dioxide (CO2).

To find the mass of butane needed to produce 79.7g of carbon dioxide, we need to calculate the molar mass of butane (C4H10) and then use stoichiometry to determine the amount of butane needed.

Step 1: Calculate the molar mass of butane (C4H10).
To calculate the molar mass, we sum up the atomic masses of each element in the compound:
C4H10:
(4 atoms of carbon x atomic mass of carbon) + (10 atoms of hydrogen x atomic mass of hydrogen)

The atomic masses (in g/mol) are:
Carbon (C): 12.01 g/mol
Hydrogen (H): 1.01 g/mol

Molar mass of C4H10 = (4 x 12.01) + (10 x 1.01) g/mol.

Step 2: Convert grams of CO2 to moles.
Using the molar mass of carbon dioxide (CO2) and the given mass, we can convert the grams of CO2 to moles:
Molar mass of CO2 = (atomic mass of carbon x 1) + (2 x atomic mass of oxygen)
Molar mass of CO2 = (12.01 g/mol x 1) + (2 x 16.00 g/mol)

Now, divide the given mass of CO2 (79.7g) by the molar mass of CO2 to obtain the number of moles of CO2.

Step 3: Use stoichiometry to determine the moles of butane.
Finally, refer to the balanced chemical equation provided:
2C4H10 + 13O2 → 10H2O + 8CO2

From the equation, we can see that 8 moles of CO2 are produced for every 2 moles of C4H10 burnt.
So, using the mol-to-mol ratio, divide the moles of CO2 calculated in Step 2 by the stoichiometric coefficient of CO2 (8) to determine the moles of C4H10 needed.

Step 4: Convert moles of butane to grams.
Multiply the moles of C4H10 by its molar mass (calculated in Step 1) to find the mass of butane needed to produce 79.7g of CO2.

Note: Make sure to use the correct number of significant figures in your final answer.

Just back track,

76.7g of CO2*(1 mole of CO2/44.01g of CO2)= moles of CO2

8 moles of CO2=2 moles of C4H10

moles of CO2*(2 moles of C4H10/8 moles of CO2)=moles of C4H10

moles of C4H10 *(58.12g of C4H10/mole of C4H10)= mass of C4H10

*******I did not check the balanced equation, so I am assuming that you did that part correctly.