One mole of an ideal gas is compressed from 500 cm 3 against a constant external pressure of 1 . 2 × 10 5 Pa . The work involved in the process is 36 . 0 J . Calculate the final volume. 200 cm 3

An ideal gas is defined as one in which all collisions between atoms or molecules are perfectly elastic and in which there are no intermolecular attractive forces. Given, The initial volume, V 1 = 500 cm 3 = 0 . 5 dm 3 . The external pressure, P ex = 1 . 2 × 10 5 Pa = 1 . 2 bar ; W = 36 J . 1 dm 3 bar = 100 J ; V 2 = ? W = - P ex V 2 - V 1 . 36 J = - 1 . 2 V 2 - 0 . 5 dm 3 bar . 36 J = - 1 . 2 × 100 V 2 - 0 . 5 J . ∴ V 2 - 0 . 5 = - 36 1 . 2 × 100 = - 0 . 3 . ∴ V 2 = 0 . 5 - 0 . 3 = 0 . 2 dm 3 = 200 cm 3 .

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Chemistry Standard 12>Chapter 4 - Chemical Thermodynamics>Exercises>Q 3

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12th Maharashtra Board

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What are intensive properties? Explain why density is intensive property.

Important Questions on Chemical Thermodynamics

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12th Maharashtra Board

IMPORTANT

Chemistry Standard 12>Chapter 4 - Chemical Thermodynamics>Exercises>Q 3

How much heat is evolved when $12 g$ of $CO$ reacts with ${NO}_{2}$ ? The reaction is $4 CO (g) + 2 {NO}_{2} (g) \to 4 {CO}_{2} (g) + N_{2} (g), Δ_{r} H^{°} = - 1200 kJ$ .