This question is also bonus since the current textbook does not have exercises for practice: Using the van der Waals equ

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answerhappygod
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This question is also bonus since the current textbook does not have exercises for practice: Using the van der Waals equ

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This question is also bonus since the current textbook does nothave exercises for practice:
Using the van der Waals equation (used for NON-ideal gases),calculate the pressure (in atm) of a 22.4 L vessel with 1.50 mol of chlorine gas at 300°C . The constantslisted in the table in thebook: a = 6.49L2-atm/mol2, b =0.0562 L/mol
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