Real gas Introduction – Deviation,\u00a0 Attraction force, molecules irregularities<\/p>\n
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A real gas<\/strong> is a gas that does not obey the ideal gas law<\/strong> perfectly under all conditions. Unlike ideal gases<\/strong>, real gases have intermolecular forces<\/strong>, and their molecules occupy a finite volume<\/strong>, leading to deviations from ideal behavior.<\/p>\n At low pressure and high temperature<\/strong>, most gases behave like ideal gases<\/strong>, but at high pressure and low temperature<\/strong>, real gases show significant deviations<\/strong> due to molecular interactions and volume effects.<\/p>\n PV=nRTPV = nRT<\/span>P<\/span>V<\/span>=<\/span><\/span>n<\/span>RT<\/span><\/span><\/span><\/span><\/span><\/p>\n However, real gases deviate due to the following reasons:<\/p>\n This deviation is represented by the compressibility factor (Z)<\/strong>:<\/p>\n Z=PVnRTZ = \\frac{PV}{nRT}<\/span>Z<\/span>=<\/span><\/span>n<\/span>RT<\/span>P<\/span>V<\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/span><\/p>\n Real gases experience intermolecular forces<\/strong>, which influence their behavior:<\/p>\n These forces reduce gas pressure<\/strong> as molecules attract each other, deviating from the ideal gas law.<\/p>\n Real gases exhibit the following molecular irregularities<\/strong>:<\/p>\n To account for deviation<\/strong> in real gases, Van der Waals modified the ideal gas equation:<\/p>\n (P+aV2)(V\u2212b)=RT\\left( P + \\frac{a}{V^2} \\right) (V – b) = RT<\/span>(<\/span><\/span>P<\/span>+<\/span>V<\/span>2<\/span><\/span><\/span><\/span>a<\/span><\/span>\u200b<\/span><\/span><\/span><\/span><\/span>)<\/span><\/span><\/span>(<\/span>V<\/span>\u2212<\/span><\/span>b<\/span>)<\/span>=<\/span><\/span>RT<\/span><\/span><\/span><\/span><\/span><\/p>\n Where:<\/p>\n This equation improves accuracy<\/strong> in predicting gas behavior under high pressure and low temperature.<\/p>\n Real gases do not follow the ideal gas law<\/strong> under all conditions due to attractive forces, molecular volume, and irregularities<\/strong>. These factors lead to deviations that can be corrected using the Van der Waals equation<\/strong>. Understanding real gas behavior is essential in applications like liquefied gas storage, refrigeration, and chemical engineering<\/strong>.<\/p>\n Sure! Here’s a clear and student-friendly explanation of Real Gases<\/strong>, their deviation from ideal behavior<\/strong>, and the role of intermolecular forces and molecular irregularities<\/strong>:<\/p>\n A real gas<\/strong> is a gas that does not perfectly follow the ideal gas laws<\/strong> (like PV = nRT), especially under high pressure<\/strong> and low temperature<\/strong>. Unlike ideal gases, real gases have volume<\/strong> and experience intermolecular forces<\/strong>.<\/p>\n Ideal gas laws assume:<\/p>\n No intermolecular forces<\/strong> between gas molecules<\/p>\n<\/li>\n Zero volume<\/strong> of gas particles<\/p>\n<\/li>\n Perfect elastic collisions<\/strong><\/p>\n<\/li>\n<\/ol>\n However, in real gases<\/strong>:<\/p>\n Molecules do attract or repel<\/strong> each other<\/p>\n<\/li>\n Each molecule occupies space (volume)<\/strong><\/p>\n<\/li>\n Collisions may involve energy loss<\/strong><\/p>\n<\/li>\n<\/ul>\n \u2705 Real gases follow ideal behavior only at low pressure and high temperature<\/strong>.<\/p>\n<\/blockquote>\n In real gases, molecules exert:<\/p>\n Attractive forces<\/strong> (like Van der Waals forces), especially when close<\/p>\n<\/li>\n These forces pull molecules inward<\/strong>, reducing pressure on the container walls<\/p>\n<\/li>\n<\/ul>\n Effect:<\/strong><\/p>\n At low temperature\/high pressure<\/strong>, attraction causes the gas to compress more than expected<\/strong><\/p>\n<\/li>\n This leads to negative deviation<\/strong> from ideal gas laws<\/p>\n<\/li>\n<\/ul>\n Molecules are not perfect spheres<\/strong><\/p>\n<\/li>\n They may have different sizes, shapes<\/strong>, and polarities<\/strong><\/p>\n<\/li>\n Some have dipoles<\/strong> or asymmetric charge distributions<\/strong><\/p>\n<\/li>\n<\/ul>\n Impact:<\/strong><\/p>\n These irregularities increase complex interactions<\/strong><\/p>\n<\/li>\n Result in non-ideal behavior<\/strong>, especially in polar gases<\/strong> like NH\u2083 or H\u2082O<\/p>\n<\/li>\n<\/ul>\nDeviation of Real Gases from Ideal Behavior<\/strong><\/h3>\n
Ideal gases follow the ideal gas equation<\/strong>:<\/h3>\n
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Attraction Forces in Real Gases<\/strong><\/h3>\n
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Molecular Irregularities in Real Gases<\/strong><\/h3>\n
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Van der Waals Equation (Correction for Real Gases)<\/strong><\/h3>\n
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Conclusion<\/strong><\/h3>\n
Real gas Introduction – Deviation,\u00a0 Attraction force, molecules irregularities<\/a><\/h3>\n
The gas laws pV = nRT<\/a><\/h3>\n
IDEAL AND REAL GASES<\/a><\/h3>\n
Lecture 4 – Real Gases<\/a><\/h3>\n
\n\ud83e\uddea Real Gas \u2013 Introduction<\/strong><\/h2>\n
\ud83d\udcd8 What is a Real Gas?<\/strong><\/h3>\n
\n\ud83d\udcc9 Deviation from Ideal Gas Behavior<\/strong><\/h2>\n
\ud83d\udd0d Why Do Real Gases Deviate?<\/h3>\n
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\n\ud83e\uddf2 Attraction Forces Between Molecules<\/strong><\/h2>\n
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\n\ud83c\udf00 Molecular Irregularities<\/strong><\/h2>\n
What are they?<\/h3>\n
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\n\ud83d\udcca Graphical Representation (PV vs P):<\/strong><\/h2>\n
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