Multiple Choice
As the pressure in the beaker was increased, what happened to the volume of the gas, assuming temperature and amount of gas remained constant?
74
views
7. Gases
Gas Stoichiometry
Multiple Choice
At standard temperature and pressure (STP), what volume is occupied by 2.719 × 10^{13} moles of methane gas (CH_4)?
A
6.09 × 10^{14} L
B
5.44 × 10^{13} L
C
1.22 × 10^{15} L
D
2.72 × 10^{13} L
Verified step by step guidance1
Recall that at standard temperature and pressure (STP), one mole of any ideal gas occupies 22.4 liters. This is a key concept in gas laws and molar volume.
Identify the given quantity: the number of moles of methane gas, which is \(2.719 \times 10^{13}\) moles.
Use the molar volume relationship to find the total volume occupied by the gas. The formula is: \(\text{Volume} = \text{moles} \times 22.4\, \text{L/mol}\).
Substitute the given number of moles into the formula: \(\text{Volume} = 2.719 \times 10^{13} \times 22.4\) liters.
Perform the multiplication to find the volume in liters. This will give you the volume occupied by the methane gas at STP.
Related Videos
Related Practice
