Answer :
Final answer:
The minimum amount of hydrogen gas, in grams, required to completely hydrogenate 15.5 kg of 2-butene is 232 grams, hence the correct answer is c) 232 g.
Explanation:
By applying the stoichiometry of a chemical reaction to determine the amount of hydrogen gas needed for the complete hydrogenation of a given mass of 2-butene.
This type of problem is a common high school level chemistry calculation, often found in the context of stoichiometry and chemical reactions in the curriculum.
- First, we need to know the molar mass of 2-butene (C4H8). Using the periodic table, we find it to be approximately 56.11 g/mol.
- Next, we calculate how many moles of 2-butene we have in 15.5 kg (or 15500 g) by dividing the mass by the molar mass of 2-butene.
- The balanced equation for the hydrogenation of 2-butene is: C4H8 + 2H2 → C4H10. This tells us that one mole of 2-butene reacts with two moles of hydrogen gas.
- After finding the amount of moles of 2-butene, we can calculate the moles of hydrogen needed by multiplying by 2, because the stoichiometry of the reaction requires two moles of hydrogen for one mole of 2-butene.
- Finally, we find out the molar mass of hydrogen gas (H2) which is approximately 2.02 g/mol. We multiply the number of moles of hydrogen gas needed by this molar mass to find the mass in grams of hydrogen gas required.
The calculations yield the minimum amount of hydrogen gas required to completely hydrogenate 15.5 kg of 2-butene to be the amount corresponding to choice (c) 232 g.
