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: Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 760 mmHg and a

Problem

Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 760 mmHg and a temperature of 30 oC.

What would the pressure be if the can were heated to 1155 oC?

Solution

Initially, a gas in a closed container has a temperature of 30°C and a pressure of 760 mm Hg. We’re being asked to determine the pressure of the gas sample if the temperature changes to 1155°C.


Recall that the ideal gas law is:

PV=nRT


The pressure, volume, and temperature of a gas are related to the number of moles of gas and the universal gas constant:

PVT=nR


The value nR is constant. For a given moles of gas, the initial and final pressure, volume, and temperature of the gas are related by the combined gas law:

P1V1T1=P2V2T2


Since the container is closed, the volume of the gas remains constant and the combined gas law becomes:

P1T1=P2T2


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