Calculate the pressure exerted by ar for a molar volume of 0.590 l⋅mol−1 at 295 k using the van der waals equation of state. the van der waals parameters a and b for ar are 1.355 bar⋅dm^6⋅mol^(−2) and 0.0320 dm^3⋅mol^(−1), respectively.

the pressure P= 40.03 bar

Explanation:

The Van der Waals equation states that

P= R*T/(V-b) - a/V²

where

T= absolute temperature = 295 K

V= molar volume = 0.590 L/mol

R= ideal gas constant = 0.082 atm*L/mol*K

a= van der Waals parameter = 1.355 bar⋅dm⁶/mol² * (0.987 atm/bar) * (1 L²/dm⁶) = 1.337 atm ⋅L²/mol²

b= van der Waals parameter = 0.032 dm³/mol *(1 L/dm³) = 0.032 L/mol

then replacing values

P= R*T/(V-b) - a/V² = 0.082 atm*L/mol*K*295 K/( 0.590 L/mol-0.032 L/mol) -  1.337 atm ⋅L²/mol²/(0.590 L/mol)² = 39.51 atm

P= 39.51 atm / (0.987 atm/bar) = 40.03 bar

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.

c. 4.54 x 10–12 j happens to be correct