0.0076 moles of an ideal gas is at 24°C. If it is a sealed container with a volume of 86 cm3, what is the pressure of the gas?

• A. 2.4×105Pa
• B. 2.6×105Pa
• C. 2.8×105Pa
• D. 3.0×105Pa
• E. 2.2×105Pa

Answer: (E)

Verified step by step guidance

1. Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. This is necessary because the ideal gas law requires temperature in Kelvin.
2. Convert the volume from cubic centimeters to cubic meters. Since 1 m³ = 1,000,000 cm³, divide the volume in cm³ by 1,000,000 to get the volume in m³.
3. Use the ideal gas law equation, which is \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the ideal gas constant (8.314 J/(mol·K)), and \( T \) is the temperature in Kelvin.
4. Rearrange the ideal gas law equation to solve for pressure \( P \): \( P = \frac{nRT}{V} \).
5. Substitute the values for \( n \), \( R \), \( T \), and \( V \) into the equation to calculate the pressure \( P \). Ensure all units are consistent for accurate calculation.