Answer:
The pressure of H₂(g) = 741 torr
Explanation:
Given that:
The atmospheric pressure measured in the lab = 765 torr
The vapor pressure of water = 24 torr
By applying Dalton's Law of Partial Pressure :
Making The Pressure inside the tube due to the H₂(g) the subject of the formula :
we have:
= (765 -24) torr
= 741 torr
You would have 24, but check to be sure
<span>The reaction leads to carbon dioxide gas.
</span><span>It releases CO2 bubbles and leftover of sodium nitrate solution.</span>
Answer:
3.02 atm
Explanation:
Step 1: Given data
- Initial pressure (P₁): 1.36 atm
- Initial volume (V₁): 4.24 × 10² mL
- Initial temperature (T₁): 25 °C
- Final volume (V₂): 1.91 × 10² mL
- Final temperature (T₂): 25 °C
Step 2: Find the final pressure
Since the temperature is constant, we can find the final pressure using Boyle's law.
Answer:
Explanation: Covalent Bond is the bond which is formed by the sharing of electrons form one atom to another in order to complete the octet of valence shell of electrons.
The strength of the covalent bond is measured by the its dissociation energy. Higher the tightly bounded the nucleus of the 2 atoms, more energy would be require to break the bond thus higher the dissociation energy. Thus the triple bond will be requiring more of the energy to break it rather than the single bond .
For the better clarification, the data is been attached in the image below.