Multiple Choice
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?
7. Gases
The Ideal Gas Law Applications
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A 75.0 g sample of dinitrogen monoxide (N2O) is confined in a 4.12 L vessel. What is the pressure (in atm) at 205°F, assuming ideal gas behavior?
A
3.45 atm
B
2.78 atm
C
1.95 atm
D
4.12 atm
Verified step by step guidance1
Convert the temperature from Fahrenheit to Celsius using the formula: \( T(°C) = \frac{5}{9} (T(°F) - 32) \). Then, convert the temperature from Celsius to Kelvin by adding 273.15.
Calculate the number of moles of dinitrogen monoxide (N2O) using its molar mass. The molar mass of N2O is approximately 44.01 g/mol. Use the formula: \( \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \).
Use the ideal gas law equation \( PV = nRT \) to solve for the pressure \( P \). Here, \( P \) is the pressure in atm, \( V \) is the volume in liters, \( n \) is the number of moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin.
Rearrange the ideal gas law equation to solve for pressure: \( P = \frac{nRT}{V} \).
Substitute the values for \( n \), \( R \), \( T \), and \( V \) into the equation to calculate the pressure in atm.
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