All Chapters
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: The density of a gas is 1.96 g/L at STP. What would the mass of 2.00 moles of the gas be at STP?1. 87.8 g2. There is not enough information to solve.3. 44.8 g4. 0.0875 g5. 43.9 g6. 0.510 g

Solution: The density of a gas is 1.96 g/L at STP. What would the mass of 2.00 moles of the gas be at STP?1. 87.8 g2. There is not enough information to solve.3. 44.8 g4. 0.0875 g5. 43.9 g6. 0.510 g

Problem

The density of a gas is 1.96 g/L at STP. What would the mass of 2.00 moles of the gas be at STP?

1. 87.8 g

2. There is not enough information to solve.

3. 44.8 g

4. 0.0875 g

5. 43.9 g

6. 0.510 g

Solution

We’re being asked to determine the mass of 2.00 moles of gas at standard temperature and pressure, given its density.


Recall that standard temperature and pressure (STP) is defined as 1 atm and 0 ˚C

The density of a gas is given by:


d=PMRT


where: 

P = pressure (in atm)           R = gas constant (0.08206 atm • L/mol • K)

T = temperature (in K)         M = molar mass

d = density


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