Textbook Question
Which gas sample has the greatest pressure? Assume that all the samples are at the same temperature. Explain.
7. Gases
The Ideal Gas Law Applications
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1.636 g of an unknown sulfur oxide gas, SO_x, is in a 0.5 L flask at 1 atm and 25.0 °C. Which is the most likely chemical formula of the compound?
A
SO2
B
SO
C
S2O
D
SO3
Verified step by step guidance1
First, use the ideal gas law equation to find the number of moles of the gas. The ideal gas law is given by: , where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin.
Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature: .
Rearrange the ideal gas law to solve for n (number of moles): . Substitute the known values: P = 1 atm, V = 0.5 L, R = 0.0821 L·atm/mol·K, and T in Kelvin.
Calculate the molar mass of the unknown gas using the formula: , where m is the mass of the gas (1.636 g) and n is the number of moles calculated in the previous step.
Compare the calculated molar mass with the molar masses of the given sulfur oxides (SO, SO2, S2O, SO3) to determine which formula matches the calculated molar mass. The closest match will be the most likely chemical formula of the compound.
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