Explanation:
The reaction is as follows.
As, value of 
is positive. Therefore, reaction is non-spontaneous.
= [-137.2 - (127.2 kJ/mol)]
= -10 kJ/mol
Since, value of is negative here so, reaction is spontaneous.
Also, = -RT ln
where, R = 8.314 J/mol K
T = 
= (400 + 273) K = 673 K
K = equilibrium constant
100 = 
log K = 0.00776
K = 1.018
Therefore, we can conclude that equilibrium constant for the coupled reaction is 1.018.
Answer:
"statement 2" for the first pair and "statement 1" for the second pair
Explanation:
The given thermochemical reaction is between hydrogen gas and chlorine gas to form hydrogen chloride.
This can be represented as:
Δ
=-184.6 kJ/mol
So when two moles of HCl is formed, 184.6 kJ of energy is released.
Calculating the heat released when 3.18 mol HCl (g) is formed in the reaction:
Therefore, 293.5 kJ of heat is released when 3.18 mol HCl is formed in the reaction between hydrogen and chlorine.
The answer is unrestrained hair.
Have a nice day!
