Equation of state of a perfect gas, work done on compressing a gas - One Line Questions
1.
The work done on a gas during compression is given by -∫ P dV. If the pressure is constant, P, and the volume changes from V1 to V2, the work done on the gas is: —
-P(V2 - V1)
2.
What is the work done on a gas during an isochoric process where the volume is constant? —
0
3.
What is the work done on a gas when it is compressed from 8 L to 2 L at a constant pressure of 5 atm? —
30 L·atm
4.
What is the work done on a gas when it is compressed from 10 L to 5 L at a constant pressure of 1 atm? —
5 L·atm
5.
If a gas is compressed from 10 m³ to 5 m³ at a constant pressure of 100 kPa, what is the work done on the gas in Joules? —
500,000 J
6.
If a gas is compressed from 5 L to 2 L at a constant pressure of 2 atm, what is the work done on the gas in L·atm? —
6 L·atm
7.
What is the value of the universal gas constant (R) in SI units (J/mol·K)? —
8.314
8.
What is the work done on a gas compressed from 4 L to 1 L at a constant pressure of 3 atm? —
9 L·atm
9.
Which process involves no heat exchange with the surroundings? —
Adiabatic
10.
For a given change in volume, which process requires the most work done *on* the gas for compression? —
Adiabatic
11.
A gas is compressed from 10 L to 5 L. If this process is done rapidly, it is likely to be closer to which type of process? —
Adiabatic
12.
Work done on a gas during adiabatic compression is always accompanied by: —
An increase in internal energy
13.
Which gas law directly relates the number of moles of a gas to its volume at constant temperature and pressure? —
Avogadro's Law
14.
The equation of state for a perfect gas can also be written as PV = NkBT, where kB is: —
Boltzmann constant
15.
In the equation PV = nRT, if n and T are constant, then PV = constant. This is a statement of: —
Boyle's Law
16.
The equation of state for a perfect gas is derived from which two gas laws? —
Boyle's Law and Charles's Law
17.
Which of the following is NOT a fundamental assumption of the kinetic theory of gases that leads to the ideal gas law? —
Intermolecular forces are attractive and significant.
18.
The equation of state PV = nRT is valid for: —
Ideal gases only
19.
The work done on a gas during an isothermal process is given by W = nRT ln(V1/V2). If the temperature (T) is increased, for the same initial and final volumes, the work done on the gas will: —
Increase
20.
The work done in compressing a gas isothermally is W = nRT ln(V1/V2). If the number of moles (n) increases, what happens to the work done for the same compression ratio? —
Increases
21.
In the formula for isothermal work done, W = nRT ln(V1/V2), what does V1 represent? —
Initial volume
22.
Which of the following conditions must be met for a gas to be considered 'ideal'? —
Intermolecular forces are negligible and molecular volume is negligible compared to the volume of the container.
23.
If the temperature of an ideal gas is kept constant, and its volume is halved, what happens to its pressure? —
It doubles
24.
If the pressure of an ideal gas is kept constant, and its absolute temperature is doubled, what happens to its volume? —
It doubles
25.
When a gas is compressed adiabatically, what happens to its temperature? —
It increases
26.
What is the unit of work done in the context of gas compression in SI units? —
Joule (J)
27.
The work done on compressing a gas is given by the integral ∫ P dV. During compression, dV is: —
Negative
28.
Consider a gas compressed from V1 to V2 (V2 < V1) at constant temperature. The work done *by* the gas is: —
Negative
29.
The work done by a gas during expansion is positive. Therefore, the work done *on* the gas during compression is: —
Negative
30.
What is the work done in compressing a gas from volume V1 to V2 (V2 < V1) isothermally? —
nRT ln(V1/V2)
31.
Boyle's Law states that for a fixed mass of gas at constant temperature, pressure is inversely proportional to volume. Mathematically, this is expressed as: —
P ∝ 1/V
32.
What is the work done when a gas is compressed isobarically (at constant pressure) from volume V1 to V2? —
P(V1 - V2)
33.
If a gas expands from V1 to V2 (V2 > V1) at constant pressure P, the work done *by* the gas is: —
P(V2 - V1)
34.
For work done *on* a gas during compression, the work done is typically considered: —
Positive
35.
If a gas is compressed such that its volume decreases, the work done *on* the gas is generally: —
Positive
36.
In the isothermal compression formula W = nRT ln(V1/V2), if V1 > V2, the term ln(V1/V2) is: —
Positive
37.
What is the ideal gas law that relates pressure, volume, temperature, and the number of moles of a gas? —
PV = nRT
38.
For a fixed amount of gas, which of the following is constant? —
PV/T
39.
What is the relationship between pressure (P), volume (V), and absolute temperature (T) for a fixed amount of an ideal gas? —
PV/T = constant
40.
What is the relationship between the universal gas constant (R) and the Boltzmann constant (kB)? —
R = NA * kB, where NA is Avogadro's number
41.
If a gas is compressed isothermally, its internal energy: —
Remains constant
42.
During an isothermal compression of an ideal gas, heat is: —
Removed from the gas
43.
For an ideal gas, the internal energy depends only on: —
Temperature
44.
In the ideal gas law PV = nRT, what does 'R' represent? —
The universal gas constant
45.
If the volume of a gas is reduced by half at constant temperature, the new pressure will be: —
Twice the original pressure
46.
Avogadro's Law states that equal volumes of all gases, at the same temperature and pressure, have the same number of molecules. This implies: —
V ∝ n (at constant P and T)
47.
Charles's Law states that for a fixed mass of gas at constant pressure, volume is directly proportional to its absolute temperature. Mathematically, this is expressed as: —
V ∝ T
48.
What is the work done when a gas is compressed isothermally from an initial volume V1 to a final volume V2? —
W = nRT ln(V1/V2)
49.
What does the area under the P-V curve represent? —
Work done
50.
If a gas is compressed at constant volume (isochoric process), what is the work done on the gas? —
Zero