At standard temperature and pressure (STP), 5.00 mol of an ideal gas occupies approximately what volume in liters?

• A. 5.00 L
• B. 22.4 L
• C. 44.8 L
• D. 112 L

Answer: (D)

Verified step by step guidance

1. Recall that at standard temperature and pressure (STP), one mole of an ideal gas occupies a volume of 22.4 liters. This is a key concept in gas laws and molar volume.
2. Write down the relationship between moles and volume at STP: \(V = n \times 22.4\, \text{L/mol}\), where \(V\) is the volume in liters and \(n\) is the number of moles.
3. Substitute the given number of moles, \(n = 5.00\), into the equation: \(V = 5.00 \times 22.4\, \text{L}\).
4. Multiply the values to find the total volume occupied by 5.00 moles of the gas at STP.
5. Interpret the result to select the correct volume from the given options, understanding that the volume scales linearly with the number of moles for an ideal gas at STP.