Answer:
<span>A 3.1 L sample of hydrogen at the same temperature and pressure contains the same number of molecules.
Explanation:
As we know ;"1 mole of any gas at STP occupies exactly 22.4 L of volume". Therefore, CO</span>₂ and H₂ gas having same number of moles (0.20 moles) will occupy exactly the same volume.
Now, converting moles into number of molecules,
# of Molecules = Moles × 6.022 × 10²³
Putting value of mole,
# of Molecules = 0.2 mol × 6.022 × 10²³ molecules.mol⁻¹
# of Molecules = 1.20 × 10²³ molecules
Hence, both gases will contain 1.20 × 10²³ molecules.
Answer:
128
Explanation:
because you multiply them
Answer:
The correct answer is "Increased energy enables more particles to collide."
Explanation:
The reaction rate is defined as the change in the concentration of one of the reagents or products, in a time interval in which the change takes place.
For a chemical reaction to take place, the molecules of the reagents must collide, and must also collide effectively. In other words, these shocks must be produced with sufficient energy so that they can break and form chemical bonds. In the crash there must be proper orientation.
When increasing the temperature, the molecules will possess greater kinetic energy, which is that energy related to the movement of the molecules. Consequently, these molecules will move faster.Thus, the possibility of colliding with another molecule increases significantly. In this way, the reaction rate increases.
So, <u><em>the correct answer is "Increased energy enables more particles to collide."</em></u>
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<span>3O2(g) <--> 2O3(g);
Keq = 1 = [O3]^2/[O2]^3
So [O2]^3 = [O3]^2
Thus A) is correct</span>
