Multiple Choice
What is the density (in g/L) of carbon dioxide gas at STP, given that the molar volume of a gas at STP is 22.4 L/mol?
7. Gases
The Ideal Gas Law: Density
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What is the temperature of a gas with a molar mass of 2.0 g/mol that has a density of 2.00 g/L and a pressure of 44.8 atm, using the Ideal Gas Law?
A
100 K
B
273 K
C
150 K
D
546 K
Verified step by step guidance1
Start by recalling the Ideal Gas Law, which is expressed as: , where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.
To find the temperature, rearrange the Ideal Gas Law to solve for T : .
Since the density of the gas is given, use the relationship between density, molar mass, and volume: , where d is density, m is mass, and V is volume. Rearrange to find V : .
Substitute the given density (2.00 g/L) and molar mass (2.0 g/mol) into the equation to find the volume of 1 mole of gas: L.
Now, substitute the values for P (44.8 atm), V (calculated volume), n (1 mole), and R (0.0821 L·atm/mol·K) into the rearranged Ideal Gas Law to solve for T .
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