balloon is filled with 1.50 L of helium gas at sea level, 1.00 atm and 32°C. The balloon is released and it rises to an altitude of 30,000 ft. If the pressure at this altitude is 0.300 atm and the temperature is −45°C, calculate the following: Initial temperature of He (KEEP ALL decimal places in converted answer) = _______ K Final temperature of He (KEEP ALL decimal places in converted answer) =_______ K Volume of the balloon at 30,000 ft (to the correct # of SFs) =______L
balloon is filled with 1.50 L of helium gas at sea level, 1.00 atm and 32°C. The balloon is released and it rises to an altitude of 30,000 ft. If the pressure at this altitude is 0.300 atm and the temperature is −45°C, calculate the following: Initial temperature of He (KEEP ALL decimal places in converted answer) = _______ K Final temperature of He (KEEP ALL decimal places in converted answer) =_______ K Volume of the balloon at 30,000 ft (to the correct # of SFs) =______L
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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A balloon is filled with 1.50 L of helium gas at sea level, 1.00 atm and 32°C. The balloon is released and it rises to an altitude of 30,000 ft. If the pressure at this altitude is 0.300 atm and the temperature is −45°C, calculate the following:
Initial temperature of He (KEEP ALL decimal places in converted answer) = _______ K
Final temperature of He (KEEP ALL decimal places in converted answer) =_______ K
Volume of the balloon at 30,000 ft (to the correct # of SFs) =______L
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