1. A chemist is preparing to carry out a reaction at high pressure that requires 36.0 mol of hydrogen gas (H2). The chemist pumps the hydrogen gas into a 12.3-L rigid steel container at 25°C. To what pressure (in atm) must the hydrogen be compressed? What would be the density of the high-pressure hydrogen?
1. A chemist is preparing to carry out a reaction at high pressure that requires 36.0 mol of hydrogen gas (H2). The chemist pumps the hydrogen gas into a 12.3-L rigid steel container at 25°C. To what pressure (in atm) must the hydrogen be compressed? What would be the density of the high-pressure hydrogen?
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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GAS LAWS
1. A chemist is preparing to carry out a reaction at high pressure that requires 36.0 mol of
hydrogen gas (H2). The chemist pumps the hydrogen gas into a 12.3-L rigid steel container
at 25°C. To what pressure (in atm) must the hydrogen be compressed? What would be the
density of the high-pressure hydrogen?
2. Calculate the molecular weight of a gaseous element if 0.480 g of gas occupies 367 mL at
0.48 atm and 45°C. Suggest the identity of the element.
3. A weather balloon is filled to the volume of 150.L on a day when the temperature is 19°C. If
no gases escaped, what would be the volume of the weather balloon after it rises to an
altitude where the temperature is -8°C?
4. Consider the following chemical reaction:
heat
KNO3-
> KNO2(s) + O2)
What mass of KNO: would have to be decomposed to produce 12.1 L of oxygen measured
at STP?
LOU
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