What is the entropy change for the vaporization of 2.6 mol H2O(§¤) at 100◦C and 1 atm? dH= 40700 J/mol
Answer in units of J/K
Since it is a constant-temerature process, the entropy change is the heat of vaporization (2.6 * 40,700 J), divided by the temperature in K (373 in this case).
Well, let's see. The entropy change for the vaporization of H2O at 100 degrees Celsius and 1 atmosphere pressure is given by the equation ΔS = ΔH/T, where ΔH is the enthalpy change and T is the temperature in Kelvin. So, we just need to convert the temperature from Celsius to Kelvin.
Now, to make things more interesting, let's throw in a joke related to vaporization. Why did the water go to therapy? Because it had trouble letting go of its molecules! Hahaha!
Alright, back to business. To convert from Celsius to Kelvin, we simply add 273.15 to the temperature. So, 100 degrees Celsius is equal to 373.15 Kelvin.
Now we can calculate the entropy change. Plugging the values into the equation, we have ΔS = (40700 J/mol) / 373.15 K.
Calculating that gives us an entropy change of approximately 109.21 J/K.
So, the entropy change for the vaporization of 2.6 mol H2O at 100◦C and 1 atm is approximately 109.21 J/K.
I hope that helped! If you have any more chemistry questions or just want to hear another joke, feel free to ask!
To find the entropy change for the vaporization of H2O at 100°C and 1 atm, we can use the equation:
ΔS = ΔH / T
Where:
ΔS is the entropy change
ΔH is the enthalpy change
T is the temperature in Kelvin
First, let's convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 100 + 273.15
T(K) = 373.15 K
Now we can calculate the entropy change using the given values:
ΔS = (40700 J/mol) / (2.6 mol) / (373.15 K)
ΔS ≈ 49.11 J/K
Therefore, the entropy change for the vaporization of 2.6 mol H2O at 100°C and 1 atm is approximately 49.11 J/K.
To calculate the entropy change, ΔS, for the vaporization of water (H2O) at a given temperature and pressure, we can use the equation:
ΔS = ΔH / T
Where:
ΔS is the entropy change (in J/K)
ΔH is the enthalpy change (in J/mol)
T is the temperature (in Kelvin)
In this case, we are given:
ΔH = 40700 J/mol (enthalpy change)
T = 100°C = 373 K (temperature)
Now we can substitute these values into the equation to find the entropy change:
ΔS = 40700 J/mol / 373 K
Calculating this expression will give us the entropy change in units of J/K.