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\( 14.0 \) moles of gas are in a \( 7.00 \mathrm{~L} \) tank at \( 24.6{ }^{\circ} \mathrm{C} \). Calculate the difference in pressure between methane and an ideal gas under these conditions. The van der Waals constants for methane are \( a=2.300 \mathrm{~L}^{2} \cdot \mathrm{atm} / \mathrm{mol}^{2} \) and \( b=0.0430 \mathrm{~L} / \mathrm{mol} \) Express your answer with the appropriate units.

Given, Number of mole(n) = 14.0 mol . Volume (V) = 7.0 L . Temperature (T) = 24.6°C = 297.75 K a = 2.30 L2.atm/mol2 . b = 0.0430 L/mol . We have to calculate the difference i