In the following reaction, first find how many oxygen molecules would be used to completely react with 230 grams of pentyl alcohol (C5H11OH)? Then, if exactly 1.505x10^21 carbon dioxide molecules were formed in this reaction, calculate the grams of water formed during this reaction. C5H11OH+O2 ---->CO2+H2O
230g of compound is 230/88.15 = 2.609 moles
The balanced equation is
2C5H11OH + 15O2 ----> 10CO2 + 12H2O
So, you will need 15/2 * 2.609 * 6.02*10^23 = 1.78 * 10^25 molecules of O2
1.505*10^21 = 0.0025 moles CO2
So, you'd have produced 12/10 * 0.0025 * 18.02 = 0.054 g H2O
To find out how many oxygen molecules are required to completely react with 230 grams of pentyl alcohol (C5H11OH), we need to use the balanced chemical equation for the reaction:
C5H11OH + O2 --> CO2 + H2O
From the balanced equation, we can see that the stoichiometric ratio between pentyl alcohol and oxygen is 1:O2. This means that 1 molecule of pentyl alcohol reacts with O2 molecules.
To calculate the number of oxygen molecules needed, we need to find the molar mass of C5H11OH (pentyl alcohol). Adding up the atomic masses gives:
Molar mass of C5H11OH = (5 * molar mass of C) + (11 * molar mass of H) + (1 * molar mass of O) = 88.15 g/mol
Next, we can calculate the number of moles of C5H11OH in 230 grams using the formula:
Number of moles = Mass / Molar mass
Number of moles of C5H11OH = 230 g / 88.15 g/mol = 2.61 mol
Since the stoichiometric ratio is 1:O2, we know that the same number of moles of oxygen are required. Therefore, 2.61 moles of O2 are needed.
To convert moles of O2 to molecules of O2, we use Avogadro's number, which states that 1 mole of any substance contains 6.022 x 10^23 molecules. Thus, the number of molecules of O2 is:
Number of molecules of O2 = Number of moles of O2 * 6.022 x 10^23 molecules/mol
Number of molecules of O2 = 2.61 mol * 6.022 x 10^23 molecules/mol = 1.571 x 10^24 molecules
Now, let's move on to the second part of the question.
If 1.505x10^21 carbon dioxide molecules were formed in the reaction, we want to calculate the mass of water formed.
From the balanced chemical equation, we can see that the stoichiometric ratio between CO2 and H2O is 1:H2O. This means that 1 molecule of CO2 reacts to form 1 molecule of H2O.
To calculate the number of moles of H2O formed, we use the same approach as before.
Number of moles of H2O = Number of moles of CO2 = (1.505x10^21 molecules) / (6.022 x 10^23 molecules/mol) = 2.5 x 10^-3 mol
Finally, we can calculate the mass of H2O formed using the molar mass of water, which is 18.015 g/mol.
Mass of H2O = Number of moles of H2O * Molar mass of H2O
Mass of H2O = 2.5 x 10^-3 mol * 18.015 g/mol = 4.51 x 10^-2 grams
Therefore, 4.51 x 10^-2 grams of water would be formed during this reaction.