Answer:
[tex]V_{H_2}=2.02x10^3LH_2[/tex]
Explanation:
Hello,
In this case, we must consider the original reaction:
[tex]C_5H_{12}\rightarrow C_5H_8+2H_2[/tex]
Which is a dehydrogenation reaction wherein the density of hydrogen (molar mass 2 g/mol) is 0.0899 g/L and the density of pentyne (molar mass 68 g/mol) is 0.681 g/mL. In such a way, given the formed volume of pentyne we can compute the volume of hydrogen that is produced by applying stoichiometry based on the 2:1 mole ratio between hydrogen and pentyne:
[tex]V_{H_2}=4.53x10^3LC_5H_8 *\frac{0.681gC_5H_8}{1LC_5H_8} *\frac{1molC_5H_8}{68gC_5H_8}*\frac{2molH_2}{1molC_5H_8} *\frac{2gH_2}{1molH_2}*\frac{1LH_2}{0.0899gH_2} \\\\V_{H_2}=2.02x10^3LH_2[/tex]
Best regards.
