18. Based on the data gas? Explain your reasoning Read This! n o the assumptions
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18. Based on the data gas? Explain your reasoning Read This! n o the assumptions of Ideal Gas Thcory gas molecules have no attraction towards one another. towards the motion of molecules is only in straight lines and there is no preference for in ne anothet, away from one another or into a wall of the container-theoretically. In a real the molecules do ha may have a slight preference for container ve attraction for one another through intermolecular forces moving towards one another instead of moving towards the wall of the pressure is determined by the number of times and the force with which a gas molecule col- between gas molecules affect the lides with the walls of the container, how will the attractions pressure will che observed pressure be higher or lower than that prediced by the ldeal Gas Law? Explain your reasoning. 20. As the intermolecular forces between gas molecules become stronger, will the deviation between the observed pressure and predicted pressure increase or decrease? Explain your reasoning 21. As the volume of the container gets larger and the gas molecules move farther apart on average, will the effect of intermolecular forces cause a greater or lesser deviation on the pressure of the gas? Explain your reasoning. 22. Consider the graph in Model 3. Areyour answers to Questions 19-21 supported by the data in Model 3? Provide specific evidence from the graph to justify your answer a. In Question 19, we said intermolecular forces should cause the pressure to be than predicted. Is this observed in Model 32 In Question 20, we said the deviation fom ideal presure should lecular forces get stronger. Is this observed in Model 3? as the intermo- POGIL™ Activities for AP. ChemistryExplanation / Answer
19. The actual pressure in the vessel is less than that calculated by the ideal gas equation because of the intermolecular forces. The ideal gas condition assumes that the gas molecules only collide with the walls of the container. But the presence of intermolecular forces in a real gas makes the collisons smaller and hence the actual observed pressure is lesser than that calculated by the ideal gas law.
20.As the intermolecular forces between the gases increase, the force with which the gas molecules collide with the waals of the container decreases and hence the observed pressure is lower than the predicted pressure using the ideal gas assumption.
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