How many moles of hydrogen are required to completely hydrogenate one mole of pent-1-en-3-yne?
Pent-1-en-3-yne has a triple bond and a double bond, so it can be hydrogenated to pentane by adding six moles of hydrogen gas (H2). Each double bond requires one mole of hydrogen gas to break the bond and form two single C-H bonds. Each triple bond requires two moles of hydrogen gas to break the bond and form two single C-H bonds and one single C-C bond.
Therefore, to hydrogenate one mole of pent-1-en-3-yne to pentane, we need:
- 3 moles of hydrogen gas for the triple bond (2 moles for each triple bond x 1 triple bond)
- 2 moles of hydrogen gas for the double bond (1 mole for each double bond x 2 double bonds)
- Total: 3 + 2 = 5 moles of hydrogen gas
Therefore, 5 moles of hydrogen gas are required to completely hydrogenate one mole of pent-1-en-3-yne.
Well, let's see here. To completely hydrogenate one mole of pent-1-en-3-yne, you would need a mole of moles of hydrogen. Just kidding! That would be quite a lot of moles.
In reality, you would need two moles of hydrogen to fully hydrogenate one mole of pent-1-en-3-yne. This is because each carbon-carbon triple bond in the pent-1-en-3-yne molecule requires two moles of hydrogen to break it and form a single bond. So, the answer is two moles.
To calculate the number of moles of hydrogen required to completely hydrogenate one mole of pent-1-en-3-yne, we need to compare the number of hydrogen atoms in the reactant and product.
The molecular formula for pent-1-en-3-yne is C5H6, which means it has 6 hydrogen atoms.
The hydrogenation reaction adds two hydrogen atoms to each carbon-carbon double bond:
C5H6 + x H2 -> C5H12
In this case, we are adding 4 hydrogen atoms to completely hydrogenate pent-1-en-3-yne.
Since there are 6 hydrogen atoms in one mole of pent-1-en-3-yne and we need 4 hydrogen atoms to hydrogenate it completely, the number of moles of hydrogen required can be calculated as:
(4 hydrogen atoms / 6 hydrogen atoms) * 1 mole of pent-1-en-3-yne
Simplifying this expression, we get:
(2/3) * 1 mole of pent-1-en-3-yne
Therefore, approximately 0.67 moles of hydrogen are required to completely hydrogenate one mole of pent-1-en-3-yne.
To find out how many moles of hydrogen are required to completely hydrogenate one mole of pent-1-en-3-yne, we need to understand the chemical equation for the hydrogenation reaction.
The hydrogenation of an alkyne involves the addition of hydrogen (H2) across the triple bond, resulting in the formation of a saturated hydrocarbon.
The balanced chemical equation for the hydrogenation of pent-1-en-3-yne is:
C5H8 + H2 -> C5H10
From the equation, we can see that one mole of pent-1-en-3-yne (C5H8) reacts with one mole of hydrogen (H2) to produce one mole of pent-1-ene (C5H10).
Hence, to completely hydrogenate one mole of pent-1-en-3-yne, we would require one mole of hydrogen.