Balance this combustion reaction first!
2C4H10 + 13O2 -> 8CO2 + 10H2O
0.86 moles C4H10 (13 moles O2/2 moles C4H10)
= 5.6 moles of oxygen required
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2 moles C8H18 (18 moles H/1 mole C8H18) = 36 moles of hydrogen =================
A. A balance chemical equation of burning of ethene is C2H4 + 3O2 ____ 2CO2 + 2H2O now according to balance chemical equation 1 mole of ethene burn by using 3 moles of oxygen so to burn 10 moles of ethene 3 x 10 30 moles of oxygen will be required.
To determine the number of hydrogen atoms in 2 mol of C8H18, we first need to calculate the molar mass of C8H18. Carbon has a molar mass of approximately 12 g/mol, and hydrogen has a molar mass of approximately 1 g/mol. Therefore, the molar mass of C8H18 is (812) + (181) = 114 g/mol. Next, we use Avogadro's number (6.022 x 10^23) to calculate the number of molecules in 2 mol of C8H18, which is 2 mol * 6.022 x 10^23 molecules/mol. Since there are 18 hydrogen atoms in each molecule of C8H18, the total number of hydrogen atoms in 2 mol of C8H18 is 2 mol * 6.022 x 10^23 molecules/mol * 18 atoms/molecule = 2.17 x 10^25 hydrogen atoms.
How many moles of C are needed to react with 0.490 mole SO2?
The balanced chemical equation for the combustion of propane (C3H8) is 1 C3H8 + 5 O2 -> 3 CO2 + 4 H2O. This means 5 moles of O2 are required for every 1 mole of C3H8. Calculate the moles of C3H8 in 51.6 g, then use the mole ratio to find the moles of O2 needed. Finally, convert the moles of O2 to grams.
16,875 moles of oxygen are needed.
2 moles C8H18 (18 moles H/1 mole C8H18) = 36 moles of hydrogen =================
In 5 moles of octane, C8H18, there are 40 moles of carbon atoms (5 moles octane x 8 carbon atoms) and 90 moles of hydrogen atoms (5 moles octane x 18 hydrogen atoms).
8,75 moles of oxygen are needed.
To determine how many moles of octane are present in 16.0 g, you would divide the mass of octane by its molar mass. The molar mass of octane (C8H18) is approximately 114.23 g/mol. Therefore, 16.0 g ÷ 114.23 g/mol = 0.14 moles of octane.
When 1 mole of C8H18 is burned, it forms 8 moles of CO2. Therefore, when 451 moles of C8H18 is burned, it will form 8 * 451 = 3608 moles of CO2.
The answer is 8 moles CO2.
Balanced equation: 2C8H18 + 25O2 ==> 16CO2 + 18H2Omoles of octane used: 325 g x 1 mole/114g = 2.85 moles octanemoles H2O produced: 18 moles H2O/2 moles C8H18 x 2.85 moles C8H18 = 25.65 moles H2O
A. A balance chemical equation of burning of ethene is C2H4 + 3O2 ____ 2CO2 + 2H2O now according to balance chemical equation 1 mole of ethene burn by using 3 moles of oxygen so to burn 10 moles of ethene 3 x 10 30 moles of oxygen will be required.
You need to state temperature and pressure of the gases I think, from this you can find the number of moles of both. The equation is 2H2 + O2 => 2H2O calculate the moles burned (for every 2 moles h2, 1 mole of O2 will burn.
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10 moles of nitrogen dioxide are needed to react with 5,0 moles of water.