7. In this experiment, after the reaction went to completion, we let the solutions sit to equilibrate the temperature in flasks A and B. If you did not do this and the gas temperature was too high (in the reaction flask A) when you measured the volume of water displaced in the reaction, would the molar volume calculated be too high or too low? Explain why. te B. Under what conditions do real gases behave most like ideal gases? Does the air in a room at room temperature (22 °C) and pressure (1 atm) behave ideally? ■. The molar volume for CO2 and HCl are 22.262 L/mol and 22.244 L/mol, respectively. Why are these molar volumes slightly less than the ideal molar volume, 22.4 L/mol?

7. In this experiment, after the reaction went to completion, we let the solutions sit to equilibrate the temperature in flasks A and B. If you did not do this and the gas temperature was too high (in the reaction flask A) when you measured the volume of water displaced in the reaction, would the molar volume calculated be too high or too low? Explain why. te B. Under what conditions do real gases behave most like ideal gases? Does the air in a room at room temperature (22 °C) and pressure (1 atm) behave ideally? ■. The molar volume for CO2 and HCl are 22.262 L/mol and 22.244 L/mol, respectively. Why are these molar volumes slightly less than the ideal molar volume, 22.4 L/mol?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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