The answer for the following question is answered below.
- <em><u>Therefore the new pressure of the gas is 1.76 atm.</u></em>
Explanation:
Given:
Initial pressure of the gas = 1.34 atm
Initial temperature of the gas = 273 K
final temperature of the gas = 312 K
To solve:
Final temperature of the gas
We know;
From the ideal gas equation
P × V = n × R × T
So;
from the above equation we can say that
<em>P ∝ T</em>
= constant
= 
Where;
= initial pressure of a gas
= final pressure of a gas
= initial temperature of a gas
= final temperature of a gas
= 
= 1.76 atm
<em><u>Therefore the new pressure of the gas is 1.76 atm.</u></em>
Hey there!
Compounds with ionic bonds have higher melting points because of the forces needed to break through the strong forces of attraction holding it together.
Compounds with covalent bonds have lower melting points because less energy is needed to break the weaker forces of attraction.
So, your answer is C. Compound 1 is ionic, and compound 2 is molecular.
Hope this helps!
Is that all you have...............................................................
This most likely means that the bonds have been broken.
The fraction of gas phase molecules is calculated by the division of final pressure to the initial pressure.
Fraction = 
(1)
Here, initial pressure = 1.0 atm
final pressure = 
First, convert torr into atm
1 atm = 760 torr
final pressure = 
= 
Now, put the value of initial and final pressure in formula (1)
Fraction = 
= 
Thus, fraction of the gas phase molecules = 
