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Physics

Chapter 1 - Electric Current, Ohms Law and Kirchhoffs Laws

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Chapter 2 - Magnetic Effects of Electric Current and Measuring Instruments

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Chapter 3 - Electromagnetic Induction and AC Dynamo and Transformer

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Chapter 4 - Alternating Current AC Circuits

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Chapter 5 - Dual Nature of Wave and Particle

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Chapter 6 - Atomic Spectra and X-Rays

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Chapter 7 - Lasers and Principles

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Chapter 8 - Modern Electronics and Semiconductors

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Quiz

Lesson 1 Quiz: Boyle, Charles, Pressure Laws and General Gas Law

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1.
Boyle's Law states that for a fixed mass of an ideal gas kept at constant temperature, the volume V is:
Directly proportional to pressure
Independent of pressure changes
Directly proportional to absolute temperature
Inversely proportional to its absolute pressure P (P1 * V1 = P2 * V2)
2.
Charles's Law establishes that at constant pressure, the volume of a given mass of gas is directly proportional to its:
Celsius temperature only
Absolute temperature in Kelvin (T_K = t_C + 273.15)
Atmospheric density
Square of the absolute temperature
3.
The volume expansion coefficient at constant pressure (alpha_v) and the pressure expansion coefficient at constant volume (beta_p) for all ideal gases have the universal constant value of:
273.15 K
1.013 x 105 Pa
8.314 J/(mol.K)
1 / 273.15 K−1 (approx. 0.00366 K−1)
4.
Absolute zero temperature (0 Kelvin or -273.15 °C) is defined physically as the theoretical temperature at which:
The volume and pressure of an ideal gas theoretically extrapolate to zero and translational molecular motion reaches its quantum minimum
Atmospheric air completely combusts
Water reaches its maximum density
All liquids solidify into glass
5.
The Ideal Gas Law combining all empirical gas relationships is mathematically formulated as:
P / V = n * R * T
P * V = m * g * h
P * V = n * R * T
P * T = n * R * V
6.
A gas cylinder contains 10 liters of gas at a pressure of 3.0 atm. If the volume is reduced to 2.5 liters at constant temperature, the new pressure inside the cylinder will be:
12.0 atm
1.2 atm
7.5 atm
6.0 atm
7.
When a gas trapped inside a rigid container of fixed volume is heated from 27 °C (300 K) to 127 °C (400 K), its pressure increases by a factor of:
4 / 3 (since P1 / T1 = P2 / T2)
2 times
127 / 27
16 / 9
8.
The universal gas constant R in SI units has the numerical value and dimensions of:
0.0821 J / mol
6.022 x 1023 J / K
1.38 x 10−23 Pa . m3
8.314 J / (mol . K)
9.
An air bubble released from the bottom of a deep lake expands in volume as it rises towards the surface because:
The water temperature at the surface is near absolute zero
The hydrostatic pressure decreases as depth decreases, allowing the trapped air to expand according to Boyle's law
Atmospheric pressure increases at the surface
The bubble absorbs water molecules into its gas phase
10.
Real gases behave most closely to an ideal gas under conditions of:
High pressure and near liquefaction point
Extremely high pressure and low temperature
Very low pressure and high temperature (where intermolecular attraction forces and molecular volumes become negligible)
Zero gravitational acceleration
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