If we apply 300 kJ of heat to 2500 moles of air at constant pressure, what is the change in internal energy?
Answer
a. 214 kJ.
b. 100 kJ.
c. 180 kJ.
d. 75 kJ.
To find the change in internal energy, we can use the equation:
ΔU = q - w
Where ΔU is the change in internal energy, q is the heat added or removed, and w is the work done on or by the system.
In this case, the heat added to the system is 300 kJ. Since the process is at constant pressure, the work done is given by the equation:
w = PΔV
Where P is the pressure and ΔV is the change in volume.
However, since we are given the number of moles of air, we can use the ideal gas law to find the change in volume:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
We can rearrange this equation to solve for ΔV:
ΔV = (nRT/P) - V
Substituting the given values: n = 2500 moles, R = ideal gas constant, T = temperature (which is not given), and P = pressure (which is not given), it seems that we are missing some key information to calculate ΔV accurately.
Therefore, we cannot determine the change in internal energy without additional information.