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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: At STP, what is the volume of 4.50 moles of nitrogen gas?A) 167 LB) 3420 LC) 101 LD) 60.7 L

Solution: At STP, what is the volume of 4.50 moles of nitrogen gas?A) 167 LB) 3420 LC) 101 LD) 60.7 L

Problem

At STP, what is the volume of 4.50 moles of nitrogen gas?

A) 167 L

B) 3420 L

C) 101 L

D) 60.7 L

Solution

We are asked to find the volume of nitrogen gas (N2) at STP. At STP, we have 273.15 K for temperature and 0.98692327 atm for pressure

Since moles, temperature, and pressure are given, we will use the ideal gas equation to calculate for the volume.


PV=nRT

P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K


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