Kinetic Molecular Theory Gas Laws - Oakland Schools

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Data Table Reaction between NH 3 and HCl Total distance between the starting marks Distance traveled by the NH 3 gas Distance traveled by the HCl gas Reaction between NaOH and HCl Total distance between the starting marks Distance traveled by the NaOH gas Distance traveled by the HCl gas Distance (cm) Distance (cm) Analysis and Conclusion Questions: 1. Write a balanced chemical equation to describe each reaction observed. 2. Give a possible reason for the location of the salt ring in each trial. 3. For each trial, calculate the ratio (acid/dbase) of the distances traveled by the gases. 4. Using the molar masses of the gases and Graham’s law, calculate the ratio of diffusion of ammonia to the diffusion rate of HCl, and the rate of diffusion of sodium hydroxide to the diffusion rate of HCl. 5. Compare the values calculated for questions 4 and 5. Are these results consistent with Graham’s law? Explain with evidence. 6. Suppose the distance between the solutions in the straw is 40.0 cm. Use Graham’s law to calculate the distance the ammonia and hydrochloric acid gases would travel before they collide. 48
Assessment Ideas Consider a balloon filled with helium and a balloon filled with air. Explain why the balloon deflates more quickly if it is filled with helium than if filled with air. Compare the rates of loss of helium from a Mylar balloon and a latex balloon. You are given a container of 1 mole of chlorine gas and 1 mole of argon gas. Both gases are at STP. Your answer choices are “chlorine”, “argon”, “both are the same”, or “neither”, and you can indicate your choice by checking the appropriate box. a. Which sample has FEWER atoms? b. Which sample has a greater mass? c. Which sample has a greater density? d. Which sample has a greater average kinetic energy? e. If there was an identical pinhole in both containers, which sample would diffuse the quickest? a. Which gas is an ideal gas? Chlorine Argon Both are the same Neither A Q-tip soaked in NH 3 and another Q-tip soaked in H 2 SO 4 are placed in opposite ends of a straw. a. Will the reaction occur closer to the NH 3 end or the H 2 SO 4 end? b. Explain why the reaction occurred near the end you chose: c. Which law did you use to determine the answer to this question? 49
Page 1 and 2: Oakland Schools Chemistry Resource
Page 3 and 4: Instructional Background Informatio
Page 5 and 6: Factor Four variables used to descr
Page 7 and 8: Kinetic Molecular Model Temperature
Page 9 and 10: Kinetic Molecular Theory and Gas La
Page 11 and 12: Calculations and Data 1. Shade in t
Page 13 and 14: Procedure/Description of Lesson 1.
Page 15 and 16: Procedures for Charles’ Law: Go t
Page 17 and 18: The math level can be upgraded by r
Page 19 and 20: Real-World Connections How do plane
Page 21 and 22: 5. Escaping Gases Effusion, mass 2
Page 23 and 24: 16. Balloon in a bottle version 2 1
Page 25 and 26: Invisible Gas Under the aquarium, t
Page 27 and 28: Reverse Gas Station Lab—CSI Style
Page 31 and 32: Real-World Connections What pressur
Page 33 and 34: 9. Notice the appearance of the aci
Page 35 and 36: Answer Key: Calculations: Calculati
Page 39 and 40: Sources Holt Chemfile C Inquiry Exp
Page 41 and 42: hot beaker, carefully fill the jar
Page 43 and 44: 12. Evaluation methods: The judge h
Page 47: Procedure: 1. On your table should

Kinetic Molecular Theory Gas Laws - Oakland Schools

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