If 1.00 mol of argon is placed in a 0.500-L container at 21.0 °C, what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345 (L2 .atm)/moland b = 0.03219 L/mol. Express your answer to two significant figures and include the appropriate units.

d.) circle motion requires a force to give it a centripetal acceleration.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24

idk what is it? is this a question that you know the answer or u dont