Question

Question 1 (1 point)

Calculate the density of nitrogen gas in a 4.32 L container at 1.0 atm and 25°C.

Question 1 options:

	0.57 g/L
	0.74 g/L
	1.15 g/L
	1.31 g/L
	1.56 g/L

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Question 2 (1 point)

What volume is occupied by 1.00 kg of nitrogen gas at 5.00?C at a pressure of 735 Torr?

Question 2 options:

	1686 L
	1242 L
	843 L
	738 L
	621 L

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Question 3 (1 point)

The ideal gas law fails to yield accurate results at low temperatures

Question 3 options:

	True
	False

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Question 4 (1 point)

The ideal gas law fails to yield accurate results at high temperatures

Question 4 options:

	True
	False

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Question 5 (1 point)

The main component of air is

Question 5 options:

	oxygen
	argon
	carbon dioxide
	nitrogen
	none of these

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Question 6 (1 point)

Gases consist mostly of

Question 6 options:

	electron clouds
	atomic nuclei
	empty space
	ions

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Question 7 (1 point)

At what temperature is the volume of an ideal gas zero?

Question 7 options:

	0°C
	-45°F
	-273 K
	-363 K
	-273°C

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Question 8 (1 point)

A real gas will behave most like an ideal gas under conditions of

Question 8 options:

	high temperature and high pressure
	high temperature and low pressure
	low temperature and high pressure
	low temperature and low pressure

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Question 9 (1 point)

If a balloon with a volume of 1.00 L pressure of 1.00 atm at 25.0?C is immersed in water at a depth where the pressure is 1.50 atm and temperature is –75.0?C what is the final volume of the balloon.

Question 9 options:

	0.443 L
	0.720 L
	1.00 L
	1.63 L
	2.26 L

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Question 10 (1 point)

5.0 moles of a gas at 1.0 atm is expanded at constant temperature from 10 L to 15 L. What is the final pressure in atm?

Question 10 options:

	1.5
	7.5
	0.67
	3.3

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Question 11 (1 point)

2.35 mol He occupies 57.9 L at 300 K and 1.00 atm. What is its volume in L at 423 K and 1.00 atm?

Question 11 options:

	0.709 L
	41.1 L
	81.6 L
	1.41 L
	57.9 L

Answer 1

Answer (1)

finding Nitrogen by ideal PV = nRT n = PV/RT P = 1atm V = 4.3L R = 0.00821Latm/ T = 25 degree c + 273.15 = 298.15 = 1 times 4.32/0.0821 times 298.15 = 0.17648moles Mas of nitrogen = moles times moles mass = 0.17648 times 14 = 2.47g Density = mass/volume = 2.47g/4.32l = 0.5719g/L = 0.57g/L