how much work is done by the system when 2.00 moles of O2 expand from a volume of 3.00 liters to a volume of 5.8 liters against a constant external pressure of 0.0100 atm? answer in units of J
work = -p*delta V
work = -0.01 atm*((5.8-3.00), then convert L*atm work to J.
1 L*atm = 101.325 J.
@sarah
To calculate the work done by the system, we can use the formula:
Work = -Pext * ΔV
Where:
- Pext is the external pressure
- ΔV is the change in volume (Vf - Vi)
First, let's calculate the change in volume:
ΔV = Vf - Vi
ΔV = 5.8 L - 3.00 L
ΔV = 2.8 L
Now we can substitute the given values into the formula:
Work = -Pext * ΔV
Work = -(0.0100 atm) * (2.8 L)
To convert atm to joules (J), we need to use the conversion factor:
1 atm = 101.325 J
So, we have:
Work = -(0.0100 atm) * (2.8 L) * (101.325 J / 1 atm)
Now we can calculate the work:
Work = -(0.0100) * (2.8) * (101.325)
Work = -2.82875 J
Since work is defined as the energy transferred to or by a system, the negative sign indicates that work is done on the system. Therefore, the work done by the system is approximately -2.83 J.