At STP, a 12.0 liter sample of CH4 (g) has the same total number of molecules as

There are four choices to choose from in regards with this problem and fortunately I know the answer to the said question:

Listed below are the choices:

a.) 6.0 L of H2 (g) at STP

b.) 12.0 L of CO2 (g) at STP

c.) 18.0 L of HCI (g) at STP

d.) 24.0 L of O2 (g) at STP

The correct answer is b. 12.0 L of CO2 (g) at STP

Note:

STP or (Standard Temperature and Pressure) - most commonly used when performing calculations on gases (e. g. gas density)

Options Given:

a. 6.0 L of H₂ (g) at STP

b. 12.0 L of CO₂ (g) at STP

c. 18.0 L of HCI (g) at STP

d. 24.0 L of O₂ (g) at STP

Answer:

Option-B is the correct answer.

Explanation:

As we know that any gas (1 mole) at standard temperature (273 K or 0 °C) and pressure (1 atm) occupies exactly 22.4 L of volume.

Therefore, at standard conditions 12 L of CH₄ containing 3.22 * 10²³ molecules will be equal to number of molecules (3.22 * 10²³) contained by 12 L of CO₂ as both the volumes are the same.