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Gas Laws & Atom Theory Quiz

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Gas Laws & Atom Theory Quiz

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Gas laws and atomic theory basics

Created by

zubia nadeem
zubia nadeem
United States

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Gas Laws & Atom Theory Quiz
 

Gas Laws & Atom Theory QuizOnline version

Gas laws and atomic theory basics

by zubia nadeem
1

Which statement best describes the law of conservation of mass?

2

What does the law of constant composition state about a pure compound?

3

Which scenario illustrates the law of multiple proportions?

4

Avogadro’s law relates which two concepts?

5

According to Gay-Lussac’s law, what happens to pressure when temperature doubles at constant volume?

6

Which statement is NOT part of Dalton’s atomic theory?

7

In a reaction, if 12 g of A and 8 g of B form products with total mass 20 g, what does this illustrate?

8

Which pair correctly reflects the law of constant composition?

9

If 22.4 L of a gas at STP contains 6.02×10^23 molecules, what is the number of molecules in the same volume of another gas at the same conditions?

10

Using Avogadro’s and ideal gas concepts, 2 moles of gas occupy how many liters at STP?

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Mass cannot be created or destroyed in a chemical reaction; it is conserved in closed systems.

Pure compounds have fixed elemental ratios by mass, regardless of sample size.

When elements form more than one compound, the masses of one element combine with a fixed mass of the other in simple whole-number ratios.

At the same temperature and pressure, equal volumes have the same number of molecules, regardless of the gas.

Pressure is directly proportional to temperature when volume is fixed.

Dalton’s model treated atoms as indivisible; later discoveries showed subatomic particles exist.

Total mass of reactants equals total mass of products in a closed system.

In any pure compound, the mass ratio of constituent elements is fixed.

At STP and same volume, equal numbers of molecules are present for any gas.

One mole at STP occupies 22.4 L; two moles occupy 44.8 L.

 
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