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Chemistry of Gases : Chemistry
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Question 1 of 34
What is the ideal gas law equation?
Choose 1 answer
PV = nRT
PV = kT
P = nRT
V = nRT
Question 2 of 34
Which gas law states that the volume of a gas is directly proportional to its temperature when pressure is constant?
Choose 1 answer
Boyle's Law
Charles's Law
Avogadro's Law
Gay-Lussac's Law
Question 3 of 34
According to Boyle's Law, what happens to the volume of a gas if the pressure is doubled, assuming temperature is constant?
Choose 1 answer
The volume doubles
The volume halves
The volume remains the same
The volume quadruples
Question 4 of 34
What is Avogadro's Law?
Choose 1 answer
Volume is directly proportional to pressure
Volume is inversely proportional to temperature
Volume is directly proportional to the number of moles
Pressure is directly proportional to temperature
Question 5 of 34
What does Gay-Lussac's Law describe?
Choose 1 answer
Relationship between volume and pressure
Relationship between volume and temperature
Relationship between pressure and temperature
Relationship between volume and number of moles
Question 6 of 34
Which of the following gases is used as a standard in gas law calculations?
Choose 1 answer
Nitrogen
Oxygen
Hydrogen
Helium
Question 7 of 34
What is the gas constant R in the ideal gas law?
Choose 1 answer
8.314 J/(mol·K)
0.0821 L·atm/(mol·K)
0.314 J/(mol·K)
1.000 L·atm/(mol·K)
Question 8 of 34
In which units should temperature be measured when using the ideal gas law?
Choose 1 answer
Celsius
Fahrenheit
Kelvin
Rankine
Question 9 of 34
What happens to the pressure of a gas if its volume is reduced to half while keeping temperature constant?
Choose 1 answer
The pressure is halved
The pressure doubles
The pressure remains the same
The pressure quadruples
Question 10 of 34
Which of the following is NOT an assumption of the ideal gas model?
Choose 1 answer
Gas molecules have no volume
Gas molecules are in constant, random motion
Gas molecules interact with each other
Collisions between gas molecules are elastic
Question 11 of 34
The term 'partial pressure' refers to:
Choose 1 answer
The pressure of a single gas in a mixture
The total pressure of the gas mixture
The pressure of the gas at standard conditions
The pressure exerted by a gas in a sealed container
Question 12 of 34
According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is:
Choose 1 answer
The sum of the partial pressures of each gas
The average of the partial pressures
The difference between the highest and lowest partial pressures
The product of the partial pressures
Question 13 of 34
What is the relationship between gas volume and the number of moles at constant temperature and pressure?
Choose 1 answer
Directly proportional
Inversely proportional
No relationship
Exponentially proportional
Question 14 of 34
Which gas law would you use to calculate the final volume of a gas when temperature changes but pressure remains constant?
Choose 1 answer
Boyle's Law
Charles's Law
Gay-Lussac's Law
Avogadro's Law
Question 15 of 34
The term 'ideal gas' refers to:
Choose 1 answer
A gas that follows all gas laws perfectly
A gas with negligible volume and no intermolecular forces
A gas at high pressure and low temperature
A gas that interacts strongly with other gases
Question 16 of 34
Which of the following gases is most likely to deviate from ideal gas behavior?
Choose 1 answer
Helium
Neon
Carbon dioxide
Hydrogen
Question 17 of 34
What effect does increasing temperature have on the pressure of a gas, if volume is held constant?
Choose 1 answer
Pressure decreases
Pressure remains constant
Pressure increases
Pressure oscillates
Question 18 of 34
In the context of the ideal gas law, what does the symbol 'n' represent?
Choose 1 answer
Pressure
Volume
Temperature
Number of moles
Question 19 of 34
What happens to the volume of a gas if the temperature is doubled while pressure remains constant?
Choose 1 answer
The volume is halved
The volume remains the same
The volume doubles
The volume quadruples
Question 20 of 34
The concept of 'elastic collisions' in gas theory means:
Choose 1 answer
Gas molecules collide without losing energy
Gas molecules lose energy upon collision
Collisions result in permanent deformation of gas molecules
Molecules absorb heat during collisions
Question 21 of 34
Which gas law is illustrated by the following equation: P1V1/T1 = P2V2/T2?
Choose 1 answer
Ideal Gas Law
Boyle's Law
Charles's Law
Combined Gas Law
Question 22 of 34
What is the value of the gas constant R when using SI units for pressure, volume, and temperature?
Choose 1 answer
8.314 J/(mol·K)
0.0821 L·atm/(mol·K)
1.000 L·atm/(mol·K)
0.314 J/(mol·K)
Question 23 of 34
Which gas law can be used to predict the behavior of a gas mixture in terms of its individual gases' pressures?
Choose 1 answer
Dalton's Law
Charles's Law
Boyle's Law
Avogadro's Law
Question 24 of 34
What does the term 'compressibility' refer to in gas chemistry?
Choose 1 answer
The ability of a gas to expand
The ability of a gas to dissolve in liquids
The ability of a gas to be reduced in volume under pressure
The ability of a gas to maintain constant pressure
Question 25 of 34
When a gas is at high pressure and low temperature, it is most likely to:
Choose 1 answer
Behave ideally
Liquefy
Expand
Increase in volume
Question 26 of 34
Which of the following is an assumption of the kinetic molecular theory of gases?
Choose 1 answer
Gas molecules have strong intermolecular forces
Gas molecules are in continuous, random motion
Gas molecules occupy a fixed volume
Gas molecules do not collide with each other
Question 27 of 34
In gas chemistry, what does 'STP' stand for?
Choose 1 answer
Standard Temperature and Pressure
Standard Time and Pressure
Standard Temperature and Partial Pressure
Standard Tension and Pressure
Question 28 of 34
Which of the following equations represents the relation between volume and temperature in Charles's Law?
Choose 1 answer
V1/T1 = V2/T2
V1P1 = V2P2
V = nRT/P
P1V1 = P2V2
Question 29 of 34
What does the term 'mole fraction' refer to in a gas mixture?
Choose 1 answer
The ratio of the number of moles of a component to the total number of moles
The ratio of the volume of a component to the total volume
The ratio of the mass of a component to the total mass
The ratio of the pressure of a component to the total pressure
Question 30 of 34
Which gas law would you use to determine the change in volume when both pressure and temperature are varied?
Choose 1 answer
Boyle's Law
Charles's Law
Ideal Gas Law
Combined Gas Law
Question 31 of 34
What is the primary limitation of the ideal gas law?
Choose 1 answer
It applies only to gases at high pressure
It assumes gas molecules do not interact
It does not account for temperature changes
It only applies to real gases
Question 32 of 34
The term 'real gas' refers to:
Choose 1 answer
A gas that follows ideal gas laws perfectly
A gas with significant intermolecular forces
A gas at low pressure and high temperature
A gas with no volume
Question 33 of 34
What is the typical value of the universal gas constant R in units of L·kPa/(mol·K)?
Choose 1 answer
8.314
0.0821
1.000
0.314
Question 34 of 34
Which gas law explains the behavior of gases at high pressures and low temperatures?
Choose 1 answer
Boyle's Law
Charles's Law
Van der Waals Equation
Ideal Gas Law
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