A pressure of 43.6 bar is required to reduce the volume of one mole of ammonia to 0.935 L at 20 Â°C.

1. What pressure would be required according to the ideal gas law?

2. What pressure would be required according to Van Der Waals' equation? [For ammonia, a=4.25 bar L^2 mol^-2 and b=0.0374 L mol^-1

3. Which of these two equation of state represents the real gas ammonia better?

4. Calculate Z at 1000 bar and 298 K using the equations in 1 and 2.

Question

A pressure of 43.6 bar is required to reduce the volume of one mole of ammonia to 0.935 L at 20 Â°C.

1. What pressure would be required according to the ideal gas law?

2. What pressure would be required according to Van Der Waals' equation? [For ammonia, a=4.25 bar L^2 mol^-2 and b=0.0374 L mol^-1

3. Which of these two equation of state represents the real gas ammonia better?

4. Calculate Z at 1000 bar and 298 K using the equations in 1 and 2.

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