An ideal gas has a volume of 5.00L under a pressure of 1.00 atm and a temperature of 10.0 K. If the temperature is changed to 10
0.0 K while the pressure is increased to 8.00 atm what would be the new volume of the gas?
6.25L
1.60L
400.0L
16.0L
6.25L
1.60L
400.0L
16.0L
1 answer:
You might be interested in
<u>Answer:</u> The for the reaction is 54.425 kJ/mol
<u>Explanation:</u>
For the given balanced chemical equation:
We are given:
To calculate for the reaction, we use the equation:
For the given equation:
Putting values in above equation, we get:
Conversion factor used = 1 kJ = 1000 J
The expression of for the given reaction:
We are given:
Putting values in above equation, we get:
To calculate the gibbs free energy of the reaction, we use the equation:
where,
= Gibbs' free energy of the reaction = ?
= Standard gibbs' free energy change of the reaction = 46900 J
R = Gas constant =
T = Temperature =
= equilibrium constant in terms of partial pressure = 20.85
Putting values in above equation, we get:
Hence, the for the reaction is 54.425 kJ/mol