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Ch.6 - Gases
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.6 - GasesProblem 81
Chapter 6, Problem 81

CH3OH can be synthesized by the reaction: CO(g) + 2 H2(g) → CH3OH( g) What volume of H2 gas (in L), at 748 mmHg and 86 °C, is required to synthesize 25.8 g CH3OH? How many liters of CO gas, measured under the same conditions, are required?

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1
Calculate the molar mass of CH3OH (methanol) using the atomic masses of carbon (C), hydrogen (H), and oxygen (O).
Determine the number of moles of CH3OH by dividing the given mass (25.8 g) by the molar mass of CH3OH.
Use the stoichiometry of the balanced chemical equation to find the moles of H2 required. According to the equation, 2 moles of H2 are needed for every mole of CH3OH produced.
Apply the ideal gas law, PV = nRT, to find the volume of H2 gas. Use the moles of H2 calculated, the given pressure (748 mmHg converted to atm), and temperature (86 °C converted to Kelvin).
Repeat the stoichiometry and ideal gas law steps for CO gas, noting that 1 mole of CO is required for every mole of CH3OH produced, and calculate the volume of CO gas under the same conditions.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It allows us to determine the amount of substances consumed and produced in a reaction. In this case, the balanced equation shows that 2 moles of H2 are needed for every mole of CH3OH produced, which is essential for calculating the required volume of H2.
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Ideal Gas Law

The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is crucial for converting the amount of H2 and CO needed, based on the stoichiometry, into volumes at the specified conditions of pressure (748 mmHg) and temperature (86 °C).
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Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. For CH3OH, the molar mass is approximately 32.04 g/mol. Knowing the molar mass allows us to convert the mass of CH3OH (25.8 g) into moles, which is necessary for using stoichiometry to find the volumes of H2 and CO required for the reaction.
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Related Practice
Textbook Question

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Consider the chemical reaction: 2 H2O(l) → 2 H2(g) + O2(g) What mass of H2O is required to form 1.85 L of O2 at a temperature of 315 K and a pressure of 0.981 atm?

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