What is the minimum amount of hydrogen gas, in grams, required to completely hydrogenate 15.5 kg of 2-butene?

Name: Chemistry: A Molecular Approach
Author: Tro
ISBN: 9780134112831

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Identify the chemical reaction involved: The hydrogenation of 2-butene (C4H8) involves adding hydrogen (H2) to convert it into butane (C4H10). The balanced chemical equation is: C4H8 + H2 -> C4H10.

Calculate the molar mass of 2-butene (C4H8) and hydrogen gas (H2). Use the atomic masses: C = 12.01 g/mol and H = 1.008 g/mol.

Determine the number of moles of 2-butene in 15.5 kg. Convert the mass from kilograms to grams, then use the molar mass of 2-butene to find the moles.

Use the stoichiometry of the balanced equation to find the moles of hydrogen gas needed. According to the equation, 1 mole of C4H8 reacts with 1 mole of H2.

Convert the moles of hydrogen gas to grams using the molar mass of H2. This will give you the minimum amount of hydrogen gas required.

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Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It allows chemists to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for determining how much hydrogen gas is needed to react with a given amount of 2-butene.

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles, which is necessary for stoichiometric calculations. For this question, knowing the molar mass of hydrogen gas (H2) and 2-butene (C4H8) will enable the calculation of the required mass of hydrogen for complete hydrogenation.

Hydrogenation Reaction

Hydrogenation is a chemical reaction that involves the addition of hydrogen (H2) to an unsaturated compound, such as alkenes or alkynes, converting them into saturated compounds. In the case of 2-butene, hydrogenation will convert it into butane. Understanding the nature of this reaction helps in determining the stoichiometric coefficients needed to calculate the amount of hydrogen required for the complete reaction.