An "empty" container is not really empty if it contains air. How many moles of nitrogen are in an "empty" two-litre cola bottle (2.00 L) at atmospheric pressure (101 kPa) and room temperature (25 °C)? Assume ideal behaviour. Express your answer to three significant figures and include the appropriate units.

Chemistry
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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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please solve part b question 4 ASAP just have less time and do not give wrong answer please

 

Review | Constants | Periodic la
Part A
What is the partial pressure of nitrogen in air at atmospheric pressure (101 kPa)? Assume ideal behaviour.
Express your answer to three significant figures and include the appropriate units.
• View Available Hint(s)
78.8 kPa
Submit
Previous Answers
v Correct
Part B
An "empty" container is not really empty if it contains air. How many moles of nitrogen are in an "empty" two-litre cola bottle (2.00 L) at atmospheric pressure (101 kPa) and room
temperature (25 °C)? Assume ideal behaviour.
Express your answer to three significant figures and include the appropriate units.
• View Available Hint(s)
Hint 1. How to approach the problem
The partial pressure of nitrogen is equal to nRT/V, where n is the number of moles of nitrogen. Therefore, by rearranging the equation we get that the number of
moles of nitrogen is equal to PV/RT, where P is the partial pressure of nitrogen.
Recall that 100 kPa = 1 bar.
Value
Units
Transcribed Image Text:Review | Constants | Periodic la Part A What is the partial pressure of nitrogen in air at atmospheric pressure (101 kPa)? Assume ideal behaviour. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) 78.8 kPa Submit Previous Answers v Correct Part B An "empty" container is not really empty if it contains air. How many moles of nitrogen are in an "empty" two-litre cola bottle (2.00 L) at atmospheric pressure (101 kPa) and room temperature (25 °C)? Assume ideal behaviour. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) Hint 1. How to approach the problem The partial pressure of nitrogen is equal to nRT/V, where n is the number of moles of nitrogen. Therefore, by rearranging the equation we get that the number of moles of nitrogen is equal to PV/RT, where P is the partial pressure of nitrogen. Recall that 100 kPa = 1 bar. Value Units
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