Calculating work, heat deltaU and deltaH for the reversible isothermal (constant temperature) expansion of 2 moles of an ideal gas from 16 Litres to 95 litres at 0 degress celcius.
*i only know how to calculate work by using this formula pressure = moles x gas constant x temp /volume then rearranging it into pressure x volume (basically work) = moles x gas constant x temp.
even so i might be wrong. so feel free to correct me,, and what about heat, deltaU and deltaH?
*i only know how to calculate work by using this formula pressure = moles x gas constant x temp /volume then rearranging it into pressure x volume (basically work) = moles x gas constant x temp.
even so i might be wrong. so feel free to correct me,, and what about heat, deltaU and deltaH?
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this is expansion isothermal. it means there is a change of volume but the temperature is constant.
1. Work
Work is defined as:
W= integral (P*dV)
As you know that
P = n*R*T/V
So,
W= integral (n*R*T/V * dV)
W= n*R*T* ln (V1/V2)
I am sure you can calculate it by yourself, but you should make all of the parameters in international system unit. (Kelvin, m^3)
2. delta U
Because it is isothermal, there is no change of temperature, it means that deltaU is zero
3. You can use fisrt law of thermodynamics
Q= deltaU + W
Q= 0 +W
Q=W
I hope it helps you
1. Work
Work is defined as:
W= integral (P*dV)
As you know that
P = n*R*T/V
So,
W= integral (n*R*T/V * dV)
W= n*R*T* ln (V1/V2)
I am sure you can calculate it by yourself, but you should make all of the parameters in international system unit. (Kelvin, m^3)
2. delta U
Because it is isothermal, there is no change of temperature, it means that deltaU is zero
3. You can use fisrt law of thermodynamics
Q= deltaU + W
Q= 0 +W
Q=W
I hope it helps you