Reduction of 1-decyne to decane requires how many equivalents of hydrogen gas?
The reduction of 1-decyne to decane requires 5 equivalents of hydrogen gas. This is because 1-decyne has one carbon-carbon triple bond that needs to be reduced to a single bond, and each triple bond requires 2 equivalents of hydrogen for reduction. Since 1-decyne has one triple bond, it requires 2 x 1 = 2 equivalents of hydrogen. Additionally, 1-decyne has 10 carbon atoms and each carbon atom requires 1 equivalent of hydrogen for reduction, so 10 x 1 = 10 equivalents of hydrogen are needed. Therefore, the total number of equivalents of hydrogen gas required is 2 + 10 = 12 equivalents.
The reduction of 1-decyne (C10H20) to decane (C10H22) requires three equivalents of hydrogen gas (H2).
To determine the number of equivalents of hydrogen gas required for the reduction of 1-decyne to decane, we need to consider the stoichiometry of the reaction.
First, let's write the balanced chemical equation for the reduction of 1-decyne to decane:
1-decyne + (2n)H2 -> decane
In this equation, "n" represents the number of equivalents of hydrogen gas required. The coefficient of H2 is multiplied by "n" to account for the number of equivalents.
Since 1 mole of H2 contains 2 equivalents of hydrogen gas, "n" equivalents of hydrogen gas correspond to "n/2" moles of H2. Therefore, we can rewrite the equation as:
1-decyne + (n/2) moles of H2 -> decane
Now, we need to determine the value of "n". Unfortunately, without further information or the complete reaction mechanism, it is not possible to determine the exact number of equivalents of hydrogen gas required for the reduction of 1-decyne to decane. The value of "n" can vary depending on the reaction conditions, catalysts, and specific reaction pathway.
If you have additional information or specific reaction conditions, it would be helpful to provide those details to estimate the number of equivalents of hydrogen gas required.