Answer:
a. 95.35 L b. 20.52 L c. 19.07 L
Explanation:
Hello,
In the attached picture, you will find the solution for this exercise.
Take into account that for the Redllich-Kwong volume, a cubic polynomial must be solved to get the roots, thus, two roots are complex and one contains the molar volume which is converted to the volume I am showing.
In the following link you will find the corresponding states graph I used: https://www.slideserve.com/taipa/che-201-introduction-to-chemical-engineering
Best regards.
Answer:
The equilibrium concentration of CH₃OH is 0.28 M
Explanation:
For the reaction: CO (g) + 2H₂(g) ↔ CH₃OH(g)
The equilibrium constant (Keq) is given for the following expresion:
Keq= 
=14.5
Where (CH3OH), (CO) and (H2) are the molar concentrations of each product or reactant.
We have:
(CH3OH)= ?
(CO)= 0.15 M
(H2)= 0.36 M
So, we only have to replace the concentrations in the equilibrium constant expression to obtain the missing concentration we need:
14.5= 
14.5 x (0.15 M) x 
= (CH₃OH)
0.2818 M = (CH₃OH)
The second gas is identified as follows
by Graham law formula
let the unknown gas be represented by letter y
=time of effusion of Neon/ time of effusion of y = sqrt (molar mass of neon/molar mass of y)
= 72 sec/ 147 sec = sqrt( 20.18 g/mol/ y g/mol)
square the both side to remove the square root sign
72^2/147^2 = 20.18 g/mol/y g/mol
=0.24 = 20.18g/mol/y g/mol
multiply both side by y g/mol
= 0.24 y g/mol = 20.18g/mol
divide both side by 0.24
y = 84 g/mol
y is therefore Krypton since it is the one with a molar mass of 84 g/mol
Answer:
Explanation:
CHECK THE ATTACHMENT FOR THE COMPLETE QUESTION AND THE DETAILED EXPLANATION
NOTE:
Equatorial atoms are referred to atoms that are attached to carbons in the cyclohexane ring which is found at the equator of the ring.
Axial atoms are atoms that exist in a bond which is parallel to the axis of the ring in cyclohexane
Answer:
For temperatures higher than 533.49 K we will see a spontaneous reaction, and for temperatures lower than that the reaction will not be spontaneous.
Explanation:
When are chemical reactions spontaneous? To find out we need to look at the reaction's change in Gibbs Free energy:
When this is greater than zero, the reaction isn't spontaneous, when it is less than zero, we have a spontaneous reaction. The reaction must then change from spontaneous to non spontaneous when 
. If we insert that into our equation we get:
That is the temperature at which the reaction's spontaneity will change, plugging in our values we find:
At that temperature we have .
Now, at a temperature greater than this one, the entropy term in our equation for the Gibbs' free energy of reaction will take over, and make 
, thus the reaction will be spontaneous.
On the other hand, if we lower the temperature, we will have a smaller entropy term, and we will have: 
. That is, the reaction will not be spontaneous. Therefore for temperatures higher than 533.49 K we will see a spontaneous reaction, and for temperatures lower than that the reaction will not be spontaneous.
