Textbook Question
Lithium reacts with nitrogen gas according to the reaction: 6 Li(s) + N2(g) → 2 Li3N(s) What mass of lithium (in g) reacts completely with 58.5 mL of N2 gas at STP?
Ch.6 - Gases
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
Not the one you use?Change textbookSelect a different textbook
Table of contents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Chapter 6, Problem 73
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?
Verified step by step guidance1
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.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
4mWas this helpful?
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.
Recommended video:
Guided course
01:16
Stoichiometry Concept
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).
Recommended video:
Guided course
01:15Ideal Gas Law Formula
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.
Recommended video:
Guided course
02:11Molar Mass Concept
Related Practice
Textbook Question
Consider the chemical reaction: 2 H2O(l) → 2 H2(g) + O2(g) What mass of H2O is required to form 1.4 L of O2 at a temperature of 315 K and a pressure of 0.957 atm?
Textbook Question
A heliox deep-sea diving mixture contains 2.0 g of oxygen to every 98.0 g of helium. What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.5 atm?
1
views
Textbook Question
Automobile air bags inflate following a serious impact. The impact triggers the chemical reaction: 2 NaN3(s) → 2 Na(s) + 3 N2(g) If an automobile air bag has a volume of 11.8 L, what mass of NaN3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.
1
views
Textbook Question
Consider the chemical reaction: C(s) + H2O(g) → CO(g) + H2(g) How many liters of hydrogen gas are formed from the complete reaction of 15.7 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 355 K.
Textbook Question
Oxygen gas reacts with powdered aluminum according to the reaction: 4 Al(s) + 3 O2(g) → 2 Al2O3(s) What volume of O2 gas (in L), measured at 782 mmHg and 25 °C, completely reacts with 53.2 g Al?